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Manual Data Processing in Analytical Chemistry: Linear Calibration Dora Melucci
Most science students are familiar with Excel spreadsheets, but determining which of Excels statistical functions perform a calculation equivalent to a classical equation and calculating errors with Excel are not trivial exercises.
Melucci, Dora. J. Chem. Educ. 2008, 85, 1346.
Calibration |
Chemometrics |
Quantitative Analysis
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Helping Students Assess the Relative Importance of Different Intermolecular Interactions Paul G. Jasien
A semi-quantitative model has been developed to estimate the relative effects of dispersion, dipoledipole interactions, and H-bonding on the normal boiling points for a series of simple, straight-chain organic compounds. Application of this model may be useful in addressing student misconceptions related to the additivity of intermolecular interactions.
Jasien, Paul G. J. Chem. Educ. 2008, 85, 1222.
Chemometrics |
Molecular Properties / Structure |
Noncovalent Interactions |
Physical Properties
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The Correlation of Binary Acid Strengths with Molecular Properties in First-Year Chemistry Travis D. Fridgen
This article replaces contradictory explanations for the strengths of different binary acids in first-year chemistry textbooks with a single explanation that uses a BornHaber cycle involving homolyic bond dissociation energies, electron affinities, and ion solvation enthalpies to rationalize trends in the strengths of all binary acids.
Fridgen, Travis D. J. Chem. Educ. 2008, 85, 1220.
Acids / Bases |
Atomic Properties / Structure |
Aqueous Solution Chemistry |
Physical Properties |
Thermodynamics
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Appreciating Oxygen Hilton M. Weiss
Photosynthetic flora and microfauna utilize light from the sun to convert carbon dioxide and water into carbohydrates and oxygen. While these carbohydrates and their derivative hydrocarbons are generally considered to be fuels, it is the thermodynamically energetic oxygen molecule that traps, stores, and provides almost all of the energy that powers life on earth.
Weiss, Hilton M. J. Chem. Educ. 2008, 85, 1218.
Bioenergetics |
Metabolism |
Oxidation / Reduction |
Photosynthesis |
Thermodynamics
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Undergraduates' Understanding of Entropy Arnd H. Jungermann
Szbilir and Bennett carried out an extensive investigation on undergraduates understanding of entropy. Though I agree in general with their statements that orderdisorder arguments form a misleading entropy concept, I would like to make some comments with regard to a certain part of their online supplement.
Jungermann, Arnd H. J. Chem. Educ. 2008, 85, 1192.
Thermodynamics
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Using Graphs of Gibbs Energy versus Temperature in General Chemistry Discussions of Phase Changes and Colligative Properties Robert M. Hanson, Patrick Riley, Jeff Schwinefus, and Paul J. Fischer
The use of qualitative graphs of Gibbs energy versus temperature is described in the context of chemical demonstrations involving phase changes and colligative properties at the general chemistry level.
Hanson, Robert M.; Riley, Patrick; Schwinefus, Jeff; Fischer, Paul J. J. Chem. Educ. 2008, 85, 1142.
Phases / Phase Transitions / Diagrams |
Physical Properties |
Thermodynamics
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Does the Addition of Inert Gases at Constant Volume and Temperature Affect Chemical Equilibrium? João C. M. Paiva, Jorge Gonçalves, and Susana Fonseca
This article examines three approaches, leading to different conclusions, for answering the question "Does the addition of inert gases at constant volume and temperature modify the state of equilibrium?"
Paiva, João C. M.; Gonçalves, Jorge; Fonseca, Susana. J. Chem. Educ. 2008, 85, 1133.
Equilibrium |
Gases |
Thermodynamics
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An Updated Equilibrium Machine Emeric Schultz
Describes a device that can demonstrate equilibrium and the Le Châtelier principle, as well as kinetic and thermodynamic concepts. The device consists of a leaf blower attached to a plastic container divided into two chambers by a barrier of variable size and form. Styrofoam balls can be exchanged across the barrier when various air pressures are applied by the blower.
Schultz, Emeric. J. Chem. Educ. 2008, 85, 1131.
Equilibrium |
Kinetics |
Thermodynamics
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An Inexpensive Solution Calorimeter Emma Kavanagh, Sam Mindel, Giles Robertson, and D. E. Peter Hughes
Describes the construction of a simple solution calorimeter, using a miniature bead thermistor as a temperature-sensing element, that has a response time of a few seconds and made it possible to carry out a thermometric reaction in under a minute.
Kavanagh, Emma; Mindel, Sam; Robertson, Giles; Hughes, D. E. Peter. J. Chem. Educ. 2008, 85, 1129.
Acids / Bases |
Aqueous Solution Chemistry |
Calorimetry / Thermochemistry |
Laboratory Equipment / Apparatus |
Thermal Analysis |
Thermodynamics
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Energy John W. Moore
Scientific Challenges in Sustainable Energy Technology, by Nathan S. Lewis of the California Institute of Technology, summarizes data on energy resources and analyses the implications for human society. Slides, text, and streaming audio/video are available at his Web site. There is much in this presentation that could (and should) be incorporated into chemistry pedagogy.
Moore, John W. J. Chem. Educ. 2008, 85, 891.
Thermodynamics
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EQVAPSIM: A Vapor–Liquid Equilibria of Binary Systems Computer Simulation by LabVIEW A. Belletti, R. Borromei, and G. Ingletto
Reports the results of a program using LabVIEW software to simulate the construction of a phase diagram representing a liquidvapor equilibrium. The program models work in a real laboratory, including mistakes commonly made in this context.
Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ. 2008, 85, 879.
Equilibrium |
Thermodynamics |
Student-Centered Learning
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Easy-To-Make Cryophoruses Rubin Battino and Trevor M. Letcher
This article describes some simple and easy-to-make cryophoruses, ideal for demonstrating evaporative cooling to students at all levels.
Battino, Rubin; Letcher, Trevor M. J. Chem. Educ. 2008, 85, 561.
Lipids |
Physical Properties |
Thermodynamics |
Liquids
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Using Pooled Data and Data Visualization To Introduce Statistical Concepts in the General Chemistry Laboratory Robert J. Olsen
This article describes how data pooling and visualization can be employed in the first-semester general chemistry laboratory to introduce core statistical concepts such as central tendency and dispersion of a data set.
Olsen, Robert J. J. Chem. Educ. 2008, 85, 544.
Chemometrics |
Stoichiometry
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Understanding the Clausius–Clapeyron Equation by Employing an Easily Adaptable Pressure Cooker Monica Galleano, Alberto Boveris, and Susana Puntarulo
Describes a laboratory exercise to understand the effect of pressure on phase equilibrium as described by the ClausiusClapeyron equation. The equipment required is a pressure cooker adapted with a pressure gauge and a thermometer in the lid, allowing the measurement of the pressure and the temperature of the chamber containing the water heated until vaporization.
Galleano, Monica; Boveris, Alberto; Puntarulo, Susana. J. Chem. Educ. 2008, 85, 276.
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Water / Water Chemistry
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A Lab Experience To Illustrate the Physicochemical Principles of Detergency J. A. Poce-Fatou, M. Bethencourt-Núñez, C. Moreno, F. J. Moreno-Dorado, and J. J. Pinto-Ganfornina
This article presents a lab to study the role of a surfactant and builder in laundry detergent efficiency as determined through measurements of the diffuse reflectances of polyester samples impregnated with linseed oil.
Poce-Fatou, J. A.; Bethencourt-Núñez, M.; Moreno, C.; Moreno-Dorado, F. J.; Pinto-Ganfornina, J. J. J. Chem. Educ. 2008, 85, 266.
Aqueous Solution Chemistry |
Consumer Chemistry |
Laboratory Equipment / Apparatus |
Micelles |
Surface Science |
Thermodynamics
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Physical Chemistry: Thermodynamics (Horia Metiu)
Taylor & Francis, New York, London, 2006. 694 pp. ISBN: 978-0815340911 (paper). $49.95Physical Chemistry: Statistical Mechanics (Horia Metiu)
Taylor & Francis, New York, London, 2006. 292 pp. ISBN: 978-0815340850 (paper). $44.95 Physical Chemistry: Kinetics (Horia Metiu)
Taylor & Francis, New York, London, 2006. 169 pp. ISBN: 978-0815340898 (paper). $44.95 Physical Chemistry: Quantum Mechanics (Horia Metiu)
Taylor & Francis, New York, London, 2006. 481 pp. ISBN: 978-0815340874 (paper). $44.95 John Krenos
Metiu has created a significant set of volumes on undergraduate physical chemistry. The integration of Mathematica and Mathcad workbooks into the four texts provides instructors with an attractive new option in teaching.
Krenos, John. J. Chem. Educ. 2008, 85, 206.
Quantum Chemistry |
Statistical Mechanics |
Thermodynamics |
Kinetics
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Reaction Order Ambiguity in Integrated Rate Plots Joe Lee
This article provides a theoretical and statistical justification for the necessity of monitoring a reaction to a substantial fraction of completion if integrated rate plots plots are to yield unambiguous orders.
Lee, Joe. J. Chem. Educ. 2008, 85, 141.
Chemometrics |
Kinetics |
Rate Law
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Introduction of Differential Scanning Calorimetry in a General Chemistry Laboratory Course: Determination of Heat Capacity of Metals and Demonstration of the Law of Dulong and Petit Ronald P. D'Amelia, Vincent Stracuzzi, and William F. Nirode
The work described herein discusses the use of differential scanning calorimetry in a general chemistry laboratory course to determine the specific heat capacities of metals and introduce the empirical law of Dulong and Petit.
D'Amelia, Ronald P.; Stracuzzi, Vincent; Nirode, William F. J. Chem. Educ. 2008, 85, 109.
Calorimetry / Thermochemistry |
Heat Capacity |
Instrumental Methods |
Thermal Analysis
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An Experimental Approach to Teaching and Learning Elementary Statistical Mechanics Frank B. Ellis and David C. Ellis
This article details demonstrations that show how equilibrium changes with temperature, energy, and entropy and involve exothermic and endothermic reactions, the dynamic nature of equilibrium, and Le Châtelier's principle.
Ellis, Frank B.; Ellis, David C. J. Chem. Educ. 2008, 85, 78.
Equilibrium |
Kinetics |
Statistical Mechanics |
Thermodynamics
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Gas Clathrate Hydrates Experiment for High School Projects and Undergraduate Laboratories Melissa P. Prado, Annie Pham, Robert E. Ferazzi, Kimberly Edwards, and Kenneth C. Janda
Presents a procedure for preparing and studying propane clathrate hydrate. This experiment introduces students to this unusual solid while stimulating a discussion of the interplay of intermolecular forces, thermodynamics, and solid structure.
Prado, Melissa P.; Pham, Annie; Ferazzi, Robert E.; Edwards, Kimberly; Janda, Kenneth C. J. Chem. Educ. 2007, 84, 1790.
Alkanes / Cycloalkanes |
Applications of Chemistry |
Calorimetry / Thermochemistry |
Gases |
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Water / Water Chemistry |
Hydrogen Bonding
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The Use of Limits in an Advanced Placement Chemistry Course Paul S. Matsumoto, Jonathan Ring, and Jia Li (Lily) Zhu
This article describes the use of limits in topics usually covered in advanced placement or first-year college chemistry. This approach supplements the interpretation of the graph of an equation since it is usually easier to evaluate the limit of a function than to generate its graph.
Matsumoto, Paul S.; Ring, Jonathan; Zhu, Jia Li (Lily). J. Chem. Educ. 2007, 84, 1655.
Acids / Bases |
Equilibrium |
Gases |
Mathematics / Symbolic Mathematics |
Thermodynamics
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Configurational Entropy Revisited Frank L. Lambert
Positional entropy should be eliminated from general chemistry instruction and replaced by emphasis on the motional energy of molecules as enabling entropy change.
Lambert, Frank L. J. Chem. Educ. 2007, 84, 1548.
Statistical Mechanics |
Thermodynamics
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The Penny Experiment Revisited: An Illustration of Significant Figures, Accuracy, Precision, and Data Analysis Joseph Bularzik
In this general chemistry laboratory the densities of pennies are measured by weighing them and using two different methods to measure their volumes. The average and standard deviation calculated for the resulting densities demonstrate that one measurement method is more accurate while the other is more precise.
Bularzik, Joseph. J. Chem. Educ. 2007, 84, 1456.
Chemometrics |
Nomenclature / Units / Symbols |
Nonmajor Courses |
Physical Properties
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Mass-Elastic Band Thermodynamics: A Visual Teaching Aid at the Introductory Level William C. Galley
Demonstrations of five spontaneous isothermal processes involving the coupling of a mass and elastic band and arising from combinations of enthalpy and entropy changes are presented and then dissected. Analogies are drawn between these processes and common spontaneous molecular events such as chemical reactions and phase transitions.
Galley, William C. J. Chem. Educ. 2007, 84, 1147.
Calorimetry / Thermochemistry |
Thermodynamics
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Peer-Developed and Peer-Led Labs in General Chemistry Lorena Tribe and Kim Kostka
Describes a student-developed and led laboratory curriculum as a model for producing a more student-centered and rich laboratory experience in general chemistry laboratories.
Tribe, Lorena; Kostka, Kim. J. Chem. Educ. 2007, 84, 1031.
Acids / Bases |
Electrochemistry |
Equilibrium |
Kinetics |
Laboratory Management |
Thermodynamics |
Student-Centered Learning
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Teaching Mathematics to Chemistry Students with Symbolic Computation J. F. Ogilvie and M. B. Monagan
The authors explain how the use of mathematical software improves the teaching and understanding of mathematics to and by chemistry students while greatly expanding their abilities to solve realistic chemical problems.
Ogilvie, J. F.; Monagan, M. B. J. Chem. Educ. 2007, 84, 889.
Chemometrics |
Computational Chemistry |
Fourier Transform Techniques |
Mathematics / Symbolic Mathematics |
Nomenclature / Units / Symbols
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Enthalpy of Vaporization and Vapor Pressures: An Inexpensive Apparatus Rubin Battino, David A. Dolson, Michael R. Hall, and Trevor M. Letcher
Describes an inexpensive apparatus for the determination of the vapor pressure of a liquid as a function of temperature for the purpose of calculating enthalpy changes of vaporization. Also described are a simple air thermostat and an inexpensive temperature controller based on an integrated temperature sensor.
Battino, Rubin; Dolson, David A.; Hall, Michael R.; Letcher, Trevor M. J. Chem. Educ. 2007, 84, 822.
Gases |
Laboratory Equipment / Apparatus |
Lipids |
Phenols |
Physical Properties |
Thermodynamics |
Liquids |
Phases / Phase Transitions / Diagrams
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"Mysteries" of the First and Second Laws of Thermodynamics Rubin Battino
Over the years the subject of thermodynamics has taken on an aura of difficulty, subtlety, and mystery. This article discusses common misconceptions and how to introduce the topic to students.
Battino, Rubin. J. Chem. Educ. 2007, 84, 753.
Calorimetry / Thermochemistry |
Thermodynamics
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Cp/Cv Ratios Measured by the Sound Velocity Method Using Calculator-Based Laboratory Technology Mario Branca and Isabella Soletta
The values ? = Cp /Cv (heat capacity at a constant pressure / heat capacity at constant volume) for air, oxygen, nitrogen, argon, and carbon dioxide were determined by measuring the velocity of sound through these gases at room temperature using Calculator-Based Laboratory Technology.
Branca, Mario; Soletta, Isabella. J. Chem. Educ. 2007, 84, 462.
Gases |
Thermodynamics |
Physical Properties
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Flame Emission Spectrometry in General Chemistry Labs: Solubility Product (Ksp) of Potassium Hydrogen Phthalate Frazier W. Nyasulu, William Cusworth III, David Lindquist, and John Mackin
In this general chemistry laboratory, flame emission spectrometry is used to determine the potassium ion concentration in saturated solutions of potassium hydrogen phthalate. From these data the solubility products, the Gibbs free energies of solution, the standard enthalpy of solution, and the standard entropy of solution are calculated.
Nyasulu, Frazier W.; Cusworth, William, III; Lindquist, David; Mackin, John. J. Chem. Educ. 2007, 84, 456.
Acids / Bases |
Atomic Properties / Structure |
Spectroscopy |
Equilibrium |
Quantitative Analysis |
Thermodynamics |
Titration / Volumetric Analysis |
Solutions / Solvents |
Aqueous Solution Chemistry |
Atomic Spectroscopy
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Introduction of Differential Scanning Calorimetry in a General Chemistry Laboratory Course: Determination of Thermal Properties of Organic Hydrocarbons Ronald DAmelia, Thomas Franks, and William F. Nirode
Differential scanning calorimetry (DSC) is a rugged, easy-to-use instrumental method for thermal analysis determinations. The work described herein discusses the use of DSC in a general chemistry laboratory course to determine thermal properties such as melting points, ?fusionH, ?fusionS, and introduce the concept of polymorphism for organic hydrocarbons.
DAmelia, Ronald; Franks, Thomas; Nirode, William F. J. Chem. Educ. 2007, 84, 453.
Alkanes / Cycloalkanes |
Instrumental Methods |
Physical Properties |
Thermal Analysis |
Thermodynamics |
Calorimetry / Thermochemistry
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Discovering the Thermodynamics of Simultaneous Equilibria. An Entropy Analysis Activity Involving Consecutive Equilibria Thomas H. Bindel
This activity explores the thermodynamics of simultaneous, consecutive equilibria and is appropriate for second-year high school or AP chemistry. Students discover that a reactant-favored (entropy-diminishing) reaction can be caused to happen if it is coupled with a product-favored reaction of sufficient entropy production.
Bindel, Thomas H. J. Chem. Educ. 2007, 84, 449.
Acids / Bases |
Equilibrium |
Thermodynamics
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Understanding Isotopic Distributions in Mass Spectrometry Juris Meija
Offers a simple graphical tool for obtaining complex isotopic distributions.
Meija, Juris. J. Chem. Educ. 2006, 83, 1761.
Mass Spectrometry |
Isotopes |
Chemometrics
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Entropy and the Shelf Model: A Quantum Physical Approach to a Physical Property Arnd H. Jungermann
A quantum physical approach relying on energy quantization leads to three simple rules which are the key to understanding the physical property described by molar entropy values.
Jungermann, Arnd H. J. Chem. Educ. 2006, 83, 1686.
Alcohols |
Alkanes / Cycloalkanes |
Carboxylic Acids |
Covalent Bonding |
Ionic Bonding |
Physical Properties |
Quantum Chemistry |
Thermodynamics
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The Importance and Efficacy of Using Statistics in the High School Chemistry Laboratory Paul S. Matsumoto
This paper describes some statistical concepts and their application to various experiments used in high school chemistry.
Matsumoto, Paul S. J. Chem. Educ. 2006, 83, 1649.
Chemometrics |
Mathematics / Symbolic Mathematics
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Job's Analysis of the Range of the "Dalton Syringe Rocket" Natalie Barto, Brandon Henrie, and Ed Vitz
An apparatus for safely igniting fuel gas/oxygen mixtures in a syringe and measuring the distance that the syringe is propelled is presented. The distance (range) is analyzed by the method of continuous variation (Job's Method) to determine the stoichiometry of the reaction.
Barto, Natalie; Henrie, Brandon; Vitz, Ed. J. Chem. Educ. 2006, 83, 1505.
Gases |
Oxidation / Reduction |
Thermodynamics |
Stoichiometry
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Dulong and Petit's Law: We Should Not Ignore Its Importance Mary Laing and Michael Laing
This article describes two student exercises: the determination of the specific heat of a metal and hence its atomic weight and a graphical study of specific heat versus atomic weight for different groups of metals and the confirmation of Dulong and Petit's law.
Laing, Mary; Laing, Michael. J. Chem. Educ. 2006, 83, 1499.
Calorimetry / Thermochemistry |
Heat Capacity |
Metals |
Periodicity / Periodic Table
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Teaching Physical Chemistry Experiments with a Computer Simulation by LabVIEW A. Belletti, R. Borromei, and G. Ingletto
This article reports on a computer simulation developed with the software LabVIEW of the physical chemistry experiment regarding the vapor pressure measurements of a pure liquid as a function of temperature, as well as a system of data collecting that emphasizes the similarities between the virtual and real experiment.
Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ. 2006, 83, 1353.
Equilibrium |
Laboratory Computing / Interfacing |
Liquids |
Thermodynamics |
Gases |
Student-Centered Learning
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Achieving Chemical Equilibrium: The Role of Imposed Conditions in the Ammonia Formation Reaction Joel Tellinghuisen
The conditions under which chemical reactions occur determine which thermodynamic functions are minimized or maximized. This point is illustrated for the formation of ammonia in the ideal gas approximation using a numerical exercise.
Tellinghuisen, Joel. J. Chem. Educ. 2006, 83, 1090.
Gases |
Equilibrium |
Thermodynamics
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Complexometric Titration of Aluminum and Magnesium Ions in Commercial Antacids. An Experiment for General and Analytical Chemistry Laboratories Shui-Ping Yang and Ruei-Ying Tsai
A novel experiment for determining the total and individual aluminum and magnesium ion content in commercial antacids is described. This experiment is developed with three independent protocols based on complexometric direct and back titrations containing the concepts and usages of blocking, masking, buffer controls and metallic indicators.
Yang, Shui-Ping; Tsai, Ruei-Ying. J. Chem. Educ. 2006, 83, 906.
Aqueous Solution Chemistry |
Chemometrics |
Consumer Chemistry |
Medicinal Chemistry |
Quantitative Analysis |
Titration / Volumetric Analysis |
UV-Vis Spectroscopy
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Intermolecular and Intramolecular Forces: A General Chemistry Laboratory Comparison of Hydrogen Bonding in Maleic and Fumaric Acids Frazier W. Nyasulu and John Macklin
This article presents a simple laboratory experiment that is designed to enhance students' understanding of inter- and intramolecular hydrogen bonding by demonstrating the comparative effect of these phenomena on some chemical and physical properties.
Nyasulu, Frazier W.; Macklin, John. J. Chem. Educ. 2006, 83, 770.
Acids / Bases |
Hydrogen Bonding |
Noncovalent Interactions |
Thermodynamics |
Titration / Volumetric Analysis
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Useful Work of a Process Norman C. Craig
Acknowledgment of a flaw in the article, Lets Drive Driving Force Out of Chemistry.
Craig, Norman C. J. Chem. Educ. 2006, 83, 703.
Bioenergetics |
Biophysical Chemistry |
Calorimetry / Thermochemistry |
Thermodynamics
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Useful Work of a Process Bruno Lunelli
Clarifies a potentially misleading statement in the article, Lets Drive Driving Force Out of Chemistry.
Lunelli, Bruno. J. Chem. Educ. 2006, 83, 703.
Bioenergetics |
Biophysical Chemistry |
Calorimetry / Thermochemistry |
Thermodynamics
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No "Driving Forces" in General Chemistry Evguenii I. Kozliak
A simple and easy-to-remember explanation, that precipitation of a solid and/or formation of water are driving forces of those reactions or drive them to completion, still occurs among instructors.
Kozliak, Evguenii I. J. Chem. Educ. 2006, 83, 702.
Bioenergetics |
Biophysical Chemistry |
Calorimetry / Thermochemistry |
Thermodynamics
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Sugar Dehydration without Sulfuric Acid Todd P. Silverstein
Offers additional solutions to the cracked watch glass problem associated with an earlier published dehydration of sugar demonstration.
Silverstein, Todd P. J. Chem. Educ. 2006, 83, 701.
Oxidation / Reduction |
Thermodynamics
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Sugar Dehydration without Sulfuric Acid Edward F. Duhr, Allison S. Soult, John G. Maijub, and Fitzgerald B. Bramwell
The procedure for Sugar Dehydration without Sulfuric Acid: No More Choking Fumes in the Classroom! can lead to watch glass breakage and thereby a fire hazard.
Duhr, Edward F.; Soult, Allison S.; Maijub, John G.; Bramwell, Fitzgerald B. J. Chem. Educ. 2006, 83, 701.
Oxidation / Reduction |
Thermodynamics
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Sugar Dehydration without Sulfuric Acid Edward F. Duhr, Allison S. Soult, John G. Maijub, and Fitzgerald B. Bramwell
The procedure for Sugar Dehydration without Sulfuric Acid: No More Choking Fumes in the Classroom! can lead to watch glass breakage and thereby a fire hazard.
Duhr, Edward F.; Soult, Allison S.; Maijub, John G.; Bramwell, Fitzgerald B. J. Chem. Educ. 2006, 83, 701.
Oxidation / Reduction |
Thermodynamics
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New Highlights on Analyzing First-Order Kinetic Data of the Peroxodisulfate–Iodide System at Different Temperatures J. Yperman and W. J. Guedens
A pseudo-first order kinetic experiment examining the peroxodisulfateiodide system is executed at different temperatures, making it possible to calculate the activation energy of this reaction.
Yperman, J.; Guedens, W. J. J. Chem. Educ. 2006, 83, 641.
Kinetics |
Laboratory Computing / Interfacing |
Oxidation / Reduction |
Rate Law |
Thermodynamics
|
Give Them Money: The Boltzmann Game, a Classroom or Laboratory Activity Modeling Entropy Changes and the Distribution of Energy in Chemical Systems Robert M. Hanson and Bridget Michalek
Described here is a short, simple activity that can be used in any high school or college chemistry classroom or lab to explore the way energy is distributed in real chemical systems and as an entry into discussions of the probabilistic nature of entropy.
Hanson, Robert M.; Michalek, Bridget. J. Chem. Educ. 2006, 83, 581.
Equilibrium |
Statistical Mechanics |
Thermodynamics
|
An Introduction to Polymer Processing, Morphology, and Property Relationships through Thermal Analysis of Plastic PET Bottles. Exercises Designed to Introduce Students to Polymer Physical Properties H. Darrell Iler, Eric Rutt, and Seth Althoff
Through thermal analyses of poly(ethylene terephthlate) (PET) bottles, students are introduced to the relationships between processing, morphology, and physical properties of polymer materials.
Iler, H. Darrell; Rutt, Eric; Althoff, Seth. J. Chem. Educ. 2006, 83, 439.
Applications of Chemistry |
Heat Capacity |
Instrumental Methods |
Materials Science |
Thermal Analysis
|
Computer Simulations of Salt Solubility Victor M. S. Gil and João C. M. Paiva
Computer Simulations of Salt Solubility provides an animated, visual interpretation of the different solubilities of related salts based on simple entropy changes associated with dissolution: configurational disorder and thermal disorder.
Gil, Victor M. S.; Paiva, João C. M. J. Chem. Educ. 2006, 83, 173.
Thermodynamics |
Equilibrium |
Solutions / Solvents |
Precipitation / Solubility |
Computational Chemistry
|
A New Java Animation in Peer-Reviewed JCE WebWare William F. Coleman and Edward W. Fedosky
Just added to JCE WebWare, Computer Simulations of Salt Solubility uses a Java applet and Web browser to present an animated illustration of differences in the solubility of salts due to differences in the entropy of solvation.
Coleman, William F.; Fedosky, Edward W. J. Chem. Educ. 2006, 83, 173.
Computational Chemistry |
Equilibrium |
Thermodynamics |
Solutions / Solvents |
Precipitation / Solubility
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Using Computer Simulations To Teach Salt Solubility. The Role of Entropy in Solubility Equilibrium Victor M. S. Gil and João C. M. Paiva
Pairs of salts are discussed to illustrate the interpretation of their different behavior in water in terms of the fundamental concept of entropy. The ability of computer simulations to help improve students' understanding of these chemistry concepts is also examined.
Gil, Victor M. S.; Paiva, João C. M. J. Chem. Educ. 2006, 83, 170.
Computational Chemistry |
Equilibrium |
Thermodynamics |
Solutions / Solvents |
Precipitation / Solubility
|
Theoretical Insights for Practical Handling of Pressurized Fluids Alfonso Aranda and María del Prado Rodríguez
Introduces the basic considerations for managing pressurized fluids, mainly liquefied and compressed gases.
Aranda, Alfonso; Rodríguez, María del Prado. J. Chem. Educ. 2006, 83, 93.
Applications of Chemistry |
Gases |
Phases / Phase Transitions / Diagrams |
Thermodynamics
|
Further Analysis of Boiling Points of Small Molecules, CHwFxClyBrz Guy Beauchamp
Multiple linear regression analysis has proven useful in selecting predictor variables that could significantly clarify the boiling point variation of the CHwFxClyBrz molecules.
Beauchamp, Guy. J. Chem. Educ. 2005, 82, 1842.
Chemometrics |
Physical Properties |
Hydrogen Bonding |
Molecular Properties / Structure |
Alkanes / Cycloalkanes
|
E = mc2 for the Chemist: When Is Mass Conserved? Richard S. Treptow
Einstein's famous equation is frequently misunderstood in textbooks and popular science literature. Its correct interpretation is that mass and energy are different measures of a single quantity known as massenergy, which is conserved in all processes.
Treptow, Richard S. J. Chem. Educ. 2005, 82, 1636.
Atomic Properties / Structure |
Nuclear / Radiochemistry |
Theoretical Chemistry |
Thermodynamics
|
A Note on Dalton's Law: Myths, Facts, and Implementation Ronald W. Missen and William R. Smith
The treatment of Dalton's law for gas mixtures commonly includes the improper designation "Dalton's law of partial pressures", rather than the correct "Dalton's law of additivity of (pure component) pressures". It also identifies the pure component pressure as the partial pressure, although these are only numerically equal for a mixture of ideal gases. The situation is clarified by examination of an appropriate statement of the law and definitions, eventually in operational form with reference to mixtures of nonideal gases.
Missen, Ronald Wi.; Smith, William R. J. Chem. Educ. 2005, 82, 1197.
Thermodynamics |
Gases
|
Equilibria That Shift Left upon Addition of More Reactant Jeffrey E. Lacy
Most textbook presentations of Le Chtelier's principle in general and physical chemistry do not include a discussion of constant pressure conditions for which addition of a reactant can shift the equilibrium to the left. We propose presentations of isothermal, open systems at constant pressure for both levels of study by using concepts and skills that the respective students already possess. In addition, we derive novel criteria based on the stoichiometry of the reaction that can be used to identify those equilibria that will shift left upon addition of more reactant.
Lacy, Jeffrey E. J. Chem. Educ. 2005, 82, 1192.
Equilibrium |
Mathematics / Symbolic Mathematics |
Thermodynamics
|
Microscopic Description of Le Châtelier's Principle Igor Novak
The analysis based on microscopic descriptors (energy levels and their populations) is given that provides visualization of free energies and conceptual rationalization of Le Châtelier's principle. The misconception "nature favors equilibrium" is highlighted.
Novak, Igor. J. Chem. Educ. 2005, 82, 1190.
Equilibrium |
Thermodynamics
|
Cross-Proportions: A Conceptual Method for Developing Quantitative Problem-Solving Skills Elzbieta Cook and Robert L. Cook
This paper focuses attention on the cross-proportion (C-P) method of mathematical problem solving, which was once widely used in chemical calculations. We propose that this method regain currency as an alternative to the dimensional analysis (DA) method, particularly in lower-level chemistry courses. In recent years, the DA method has emerged as the only problem solving mechanism offered to high-school and general chemistry students in contemporary textbooks, replacing more conceptual methods, C-P included.
Cook, Elzbieta; Cook, Robert L. J. Chem. Educ. 2005, 82, 1187.
Learning Theories |
Stoichiometry |
Chemometrics |
Student-Centered Learning
|
The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems: The Reaction Quotient (Q) IS Useful After All Todd P. Silverstein
Paul Matsumoto was absolutely correct in writing The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems.
Silverstein, Todd P. J. Chem. Educ. 2005, 82, 1149.
Equilibrium |
Thermodynamics
|
The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems: The Reaction Quotient (Q) IS Useful After All Todd P. Silverstein
Paul Matsumoto was absolutely correct in writing The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems.
Silverstein, Todd P. J. Chem. Educ. 2005, 82, 1149.
Equilibrium |
Thermodynamics
|
Conceptual Considerations in Molecular Science Donald T. Sawyer
The undergraduate curriculum and associated textbooks include several significant misconceptions.
Sawyer, Donald T. J. Chem. Educ. 2005, 82, 985.
Catalysis |
Covalent Bonding |
Electrolytic / Galvanic Cells / Potentials |
Oxidation / Reduction |
Reactions |
Reactive Intermediates |
Thermodynamics |
Water / Water Chemistry
|
JavaScript Programs To Calculate Thermodynamic Properties Using Cubic Equations of State
Cubic equations of state are widely used by chemists and chemical engineers to predict the thermodynamic properties of both pure substances and mixtures. In particular, these equations enable predictions concerning the temperature and pressure at which vaporliquid equilibrium occurs. These two educational JavaScript programs perform calculations using cubic equations of state and, equally importantly, explain how the calculations are performed.
J. Chem. Educ. 2005, 82, 960.
Enrichment / Review Materials |
Equilibrium |
Thermodynamics
|
JavaScript Programs To Calculate Thermodynamic Properties Using Cubic Equations of State Patrick J. Barrie
In this article, two JavaScript programs are described. The first program gives students the choice of five different cubic equations of state and performs calculations for pure substances. The second program predicts vaporliquid equilibrium for binary mixtures using a choice of three modern equations of state and the van der Waals mixing rules.
Barrie, Patrick J. J. Chem. Educ. 2005, 82, 958.
Enrichment / Review Materials |
Thermodynamics |
Equilibrium
|
The q/T Paradox: Which "Contains More Heat", a Cup of Coffee at 95°C or a Liter of Icewater? Ed Vitz and Michael J. Schuman
In this demonstration, heat is removed from 10 cm3 of water at ~95C and 42 cm3 of water at ~0C by adding each to a measured sample of liquid nitrogen. The heat removed from the water boils the N2(l), and the quantity of liquid nitrogen that is evaporated by boiling is determined. The quantity of heat that was absorbed is calculated from the heat of vaporization of liquid nitrogen and found to be about 10,000 J in the case of the hot water and 25,000 J in the case of the icewater.
Vitz, Ed; Schuman, Michael J. J. Chem. Educ. 2005, 82, 856.
Calorimetry / Thermochemistry |
Heat Capacity |
Phases / Phase Transitions / Diagrams |
Thermodynamics
|
Regarding Entropy Analysis Thomas H. Bindel
There is a problem with the symbol ?Suniv as it does not indicate whether the reactive system is in standard state or not.
Bindel, Thomas H. J. Chem. Educ. 2005, 82, 839.
Thermodynamics
|
Regarding Entropy Analysis Robert M. Hanson
Presents a minor criticism I have regards ?Suniv not involving entropy effects of concentration and pressure.
Hanson, Robert M. J. Chem. Educ. 2005, 82, 839.
Thermodynamics
|
Let's Drive "Driving Force" Out of Chemistry Norman C. Craig
"Driving force" is identified as a misleading concept in analyzing spontaneous change. Driving force wrongly suggests that Newtonian mechanics and determinism control and explain spontaneous processes. The usefulness of the competition of ?H versus ?S in discussing chemical change is also questioned. Entropy analyseswhich consider the contributions to the total change in entropyare advocated.
Craig, Norman C. J. Chem. Educ. 2005, 82, 827.
Natural Products |
Bioenergetics |
Biophysical Chemistry |
Calorimetry / Thermochemistry |
Thermodynamics
|
Procedure for Decomposing a Redox Reaction into Half-Reactions Ilie Fishtik and Ladislav H. Berka
The principle of stoichiometric uniqueness provides a simple algorithm to check whether a simple redox reaction may be uniquely decomposed into half-reactions in a single way. For complex redox reactions the approach permits a complete enumeration of a finite and unique number of ways a redox reaction may be decomposed into half-reactions. Several examples are given.
Fishtik, Ilie; Berka, Ladislav H. J. Chem. Educ. 2005, 82, 553.
Stoichiometry |
Equilibrium |
Electrochemistry |
Oxidation / Reduction |
Reactions |
Thermodynamics
|
The Reaction Quotient Is Unnecessary To Solve Equilibrium Problems Paul S. Matsumoto
The traditional method to determine the equilibrium concentration of chemicals in a reaction, given the equilibrium constant and the initial concentration of chemicals in the reaction, involves the determination of the reaction quotient. This article will demonstrate that this step may be eliminated; thereby simplifying the algorithm to solve such problems. Such a reduction in the complexity of the algorithm may result in more students successfully being able to solve such problems.
Matsumoto, Paul S. J. Chem. Educ. 2005, 82, 406.
Equilibrium |
Learning Theories |
Chemometrics
|
Capillary Electrophoresis Analysis of Cations in Water Samples. An Experiment for the Introductory Laboratory Christopher J. Pursell, Bert Chandler, and Michelle M. Bushey
This experiment can be done in a lab, as a "dry-lab", or as an in-class exercise. Students explore a number of basic separation topics and work with figures of merit for real and meaningful samples. We have adopted a strategy where students encounter various instruments and methods of analyses multiple times throughout the curriculum. The level of sophistication in the exposures increases with the experience level of the students. Through this repeated exposure students will gain a better and fuller understanding of these methods than they would with a single exposure to the technique in the analytical or instrumental laboratory.
Pursell, Christopher J.; Chandler, Bert; Bushey, Michelle M. J. Chem. Educ. 2004, 81, 1783.
Electrophoresis |
Quantitative Analysis |
Separation Science |
Chemometrics |
Water / Water Chemistry
|
A Pedagogical Simulation of Maxwell's Demon Paradox D. López and C. Criado
Teaching thermodynamics from the microscopic point of view can help students develop an intuitive understanding of its concepts. This program simulates, at the microscopic level, two gas chambers with an opening between them. The program allows students or their instructors to set up simulations that illustrate the thermodynamics and statistical behavior of the system. The user determines the basis for whether the demon permits or denies passage of particles through the opening using information from the microscopic level, such as specific particle velocity. Students can track and analyze how this affects particle distribution, thermal equilibrium, relaxation time, diffusion, and distribution of particle velocities.
López, D.; Criado, C. J. Chem. Educ. 2004, 81, 1679.
Statistical Mechanics |
Thermodynamics
|
Statistical Comparison of Data in the Analytical Laboratory Michael J. Samide
In this article, an experiment designed to provide students with an experience involving statistical treatment of data is described. This experiment allows students to compare 11 different techniques for measuring specific volumes of water. Replicate measurements are taken for each technique and comparisons are made both within a data set and between different data sets. Through calculation of t-values, students are able to draw conclusions about the precision and accuracy of these various techniques.
Samide, Michael J. J. Chem. Educ. 2004, 81, 1641.
Chemometrics
|
Teaching Entropy Analysis in the First-Year High School Course and Beyond Thomas H. Bindel
A 16-day teaching unit is presented that develops chemical thermodynamics at the introductory high school level and beyond from exclusively an entropy viewpoint referred to as entropy analysis. Many concepts are presented, such as: entropy, spontaneity, the second law of thermodynamics, qualitative and quantitative entropy analysis, extent of reaction, thermodynamic equilibrium, coupled equilibria, and Gibbs free energy. Entropy is presented in a nontraditional way, using energy dispersal.
Bindel, Thomas H. J. Chem. Educ. 2004, 81, 1585.
Thermodynamics
|
Campbell's Rule for Estimating Entropy Changes Norman C. Craig
I am pleased that Campbells rule for estimating entropy changes in gas-consuming and gas-producing chemical reactions has attracted immediate interest.
Craig, Norman C. J. Chem. Educ. 2004, 81, 1571.
Gases |
Thermodynamics
|
Campbell's Rule for Estimating Entropy Changes William B. Jensen
In a recent article Norman Craig has proposed the rule-of-thumb that the approximate value of the entropy of reaction is related to the net moles of gas consumed or generated in the reaction .
Jensen, William B. J. Chem. Educ. 2004, 81, 1570.
Gases |
Thermodynamics
|
Playing Card Equilibrium Frank L. Lambert
From experience, I am hypersensitive to the misconceptions of students and instructors that can be caused when playing cards are used in teaching chemistry. The root of such errors lies in overlooking the non-mobile, non-energetically-interacting nature of pieces of cardboard. Only if they are being shuffled can cards serve as some sort of analogy to molecular behavior in chemistry.
Lambert, Frank L. J. Chem. Educ. 2004, 81, 1569.
Equilibrium |
Statistical Mechanics |
Thermodynamics
|
Unified Approximations: A New Approach for Monoprotic Weak Acid–Base Equilibria Harry L. Pardue, Ihab N. Odeh, and Teweldemedhin M. Tesfai
This article describes a new approach to approximate calculations for monoprotic acidbase equilibria in otherwise pure water. The new approach, identified herein as unified approximations, uses a simple decision criterion to select between situations that should be treated as deprotonation and protonation reactions. The remaining treatment takes account of changes in concentrations of conjugate acidbase pairs for all situations and ignores autoprotolysis only for situations for which the analytical concentration of either the conjugate acid or conjugate base will always be larger than zero.
Pardue, Harry L.; Odeh, Ihab N.; Tesfai, Teweldemedhin M. J. Chem. Educ. 2004, 81, 1367.
Acids / Bases |
Equilibrium |
Chemometrics
|
Reaction to Why Do We Teach Equilibrium Calculations? Stephen J. Hawkes
"Rigor" in introductory chemistry is often equated with quantitation. Consequently the understanding of chemical reactions and properties is obscured. This was illustrated by Stumpo who asked students to calculate ?E of a reaction, and then on another question on the same test asked a question aimed at its meaning. 77% of the students calculated correctly, but only 24% showed understanding of its meaning. The ability to calculate a number does not measure understanding of the number.
Hawkes, Stephen J. J. Chem. Educ. 2004, 81, 1265.
Equilibrium |
Chemometrics
|
Reaction to Why Do We Teach Equilibrium Calculations? Don L. Lewis
A recently published correspondence by Stephen J. Hawkes on teaching equilibrium calculations troubles me. Hawkes dismisses equilibrium calculations as mere algorithms, best deferred until the student can use computer programs. I find it difficult to believe that a computer program enhances understanding. From a chemists point of view, the equilibrium condition is a limit, a limit that (because of stochastic considerations) does not exist. It might be better to make the reaction quotient statement using < or > but the use of those relations is delayed until quantum mechanics.
Lewis, Don L. J. Chem. Educ. 2004, 81, 1265.
Equilibrium |
Chemometrics
|
Entropy and Constraint of Motion Frank L. Lambert
William Jensen's presentation of entropy increase as solely due to kinetic energy dispersion is stimulating.
Lambert, Frank L. J. Chem. Educ. 2004, 81, 640.
Thermodynamics
|
Entropy and Constraint of Motion William B. Jensen
I would like to make several observations supplementing and supporting the article by Frank Lambert on entropy as energy dissipation, since this is an approach that I have also used for many years when teaching a qualitative version of the entropy concept to students of general and introductory inorganic chemistry.
Jensen, William B. J. Chem. Educ. 2004, 81, 639.
Thermodynamics
|
Using Science Fiction To Teach Thermodynamics: Vonnegut, Ice-nine, and Global Warming Charles A. Liberko
When covering the topic of thermodynamics at the introductory level, an example from Kurt Vonnegut, Jr's, fictional novel, Cat's Cradle, is used to take what the students have learned and apply it to a new situation.
Liberko, Charles A. J. Chem. Educ. 2004, 81, 509.
Thermodynamics |
Water / Water Chemistry |
Phases / Phase Transitions / Diagrams |
Noncovalent Interactions |
Calorimetry / Thermochemistry
|
Using a Graphing Calculator To Determine a First-Order Rate Constant: Author Reply José E. Cortés-Figueroa
When technology is used to help with mathematical calculations, the emphasis must be on the concepts being learned rather than simply the procedures. In our approach we are attempting to help students learn more about the concept and also to attain data analysis skills they will need in the future.
Cortés-Figueroa, José E. J. Chem. Educ. 2004, 81, 485.
Kinetics |
Chemometrics
|
Using a Graphing Calculator To Determine a First-Order Rate Constant Todd P. Silverstein
The authors use the graphing calculator to estimate the infinity reading from linearized kinetics data, and then they use linearized semi-log data to determine the first-order rate constant.
Silverstein, Todd P. J. Chem. Educ. 2004, 81, 485.
Kinetics |
Chemometrics
|
Effects of an Active Learning Environment: Teaching Innovations at a Research I Institution Maria T. Oliver-Hoyo, DeeDee Allen, William F. Hunt, Joy Hutson, and Angela Pitts
This paper describes a new approach for teaching general chemistry that combines lecture and laboratory into one seamless session and incorporates instructional methods supported by research-based findings. The results of a study that compared two instructional formats, conventional passive lecture and the student-centered, highly collaborative format known as cAcL2 (concept Advancement through chemistry LabLecture), are also presented.
Oliver-Hoyo, Maria T.; Allen, DeeDee; Hunt, William F.; Hutson, Joy; Pitts, Angela. J. Chem. Educ. 2004, 81, 441.
Chemometrics |
Student-Centered Learning
|
Thermodynamics in Context: A Case Study of Contextualized Teaching for Undergraduates John Holman and Gwen Pilling
Thermodynamics is often considered to be a dry and theoretical area of undergraduate chemistry. To make it more accessible, a contextualized approach to first-year university thermodynamics has been developed, building on the experiences at the high school level of ChemCom in the United States and Salters Advanced Chemistry in the United Kingdom.
Holman, John; Pilling, Gwen. J. Chem. Educ. 2004, 81, 373.
Thermodynamics |
Learning Theories
|
Why Chemical Reactions Happen (James Keeler and Peter Wothers) John Krenos
By concentrating on a limited number of model reactions, this book presents chemistry as a cohesive whole by tying together the fundamentals of thermodynamics, chemical kinetics, and quantum chemistry, mainly through the use of molecular orbital interpretations.
Krenos, John. J. Chem. Educ. 2004, 81, 201.
Mechanisms of Reactions |
Thermodynamics |
Kinetics |
Quantum Chemistry |
MO Theory
|
Don't Be Tricked by Your Integrated Rate Plot Edward Urbansky
Reply to comments on original article.
Urbansky, Edward. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
|
Don't Be Tricked by Your Integrated Rate Plot: Reaction order Ambiguity Sue Le Vent
Integrated rate equations (for constant reaction volume) may be given in terms of relative reactant concentration, C (= concentration/initial concentration) and relative time, T (= time/half-life); in these forms, the equations are independent of rate constants and initial concentrations.
Le Vent, Sue. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
|
Don't Be Tricked by Your Integrated Rate Plot: Pitfalls of Using Integrated Rate Plots Gabor Lente
Problems with linearizing the integrated rate law.
Lente, Gabor. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
|
Don't Be Tricked by Your Integrated Rate Plot: Pitfalls of Using Integrated Rate Plots Gabor Lente
Problems with linearizing the integrated rate law.
Lente, Gabor. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
|
Another Variation on the "Whoosh Bottle" Theme Dean J. Campbell
Additional safety considerations and a CO2 rocket car.
Campbell, Dean J. J. Chem. Educ. 2004, 81, 31.
Thermodynamics |
Gases
|
Another Variation on the "Whoosh Bottle" Theme Edward G. Senkbeil
Description of a similar demonstration and additional safety considerations.
Senkbeil, Edward G. J. Chem. Educ. 2004, 81, 31.
Thermodynamics |
Gases
|
Another Variation on the "Whoosh Bottle" Theme Edward G. Senkbeil
Description of a similar demonstration and additional safety considerations.
Senkbeil, Edward G. J. Chem. Educ. 2004, 81, 31.
Thermodynamics |
Gases
|
Playing-Card Equilibrium Robert M. Hanson
A simple hands-on simulation suitable for either classroom use or laboratory investigation involves using a standard deck of playing cards to explore the statistical aspects of equilibrium. Concepts that can be easily demonstrated include fluctuation around a most probable distribution, Le Chtelier's principle, the equilibrium constant, prediction of the equilibrium constant based on probability, and the effect of sample size on equilibrium fluctuations.
Hanson, Robert M. J. Chem. Educ. 2003, 80, 1271.
Equilibrium |
Statistical Mechanics |
Thermodynamics
|
SpecScan: A Utility Program for Generating Numerical Data from Printed Forms of Spectra or Other Signals Constantinos E. Efstathiou
SpecSpan is a utility program for Microsoft Windows that generates numerical data from printed spectra or other plots found as figures in text, chart recordings, or freehand drawings. SpecScan can process bitmap (.BMP) images of such figures and drawings. After a brief interaction with the user, it generates and exports numerical data as Excel (.XLS) or text (.TXT) files.
Efstathiou, Constantinos E. J. Chem. Educ. 2003, 80, 1093.
Chemometrics |
Spectroscopy
|
From Our Peer-Reviewed Collection William F. Coleman and Edward W. Fedosky
The JCE WebWare collection continues to evolve and grow. This month we add another program, SpecScan: A Utility Program for Generating Numerical Data from Printed Forms of Spectra or Other Signals, to our collection of peer-reviewed WebWare.
Coleman, William F.; Fedosky, Edward W. J. Chem. Educ. 2003, 80, 1093.
Chemometrics |
Spectroscopy
|
SpecScan: A Utility Program for Generating Numerical Data from Printed Forms of Spectra or Other Signals Constantinos E. Efstathiou
The JCE WebWare collection continues to evolve and grow. This month we add another program, SpecScan: A Utility Program for Generating Numerical Data from Printed Forms of Spectra or Other Signals, to our collection of peer-reviewed WebWare.
Efstathiou, Constantinos E. J. Chem. Educ. 2003, 80, 1093.
Chemometrics |
Spectroscopy
|
Two Linear Correlation Coefficients Robert de Levie
In fitting data to a straight line, many calculators and computer programs display a linear correlation coefficient. Two types of linear correlation coefficients are discussed, one often useful in chemical calculations, the other usually not.
de Levie, Robert. J. Chem. Educ. 2003, 80, 1030.
Chemometrics
|
Three Forms of Energy Sigthór Pétursson
Calculations comparing the energy involved in three forms: heat, mechanical energy, and expansion against pressure.
Pétursson, Sigthór . J. Chem. Educ. 2003, 80, 776.
Calorimetry / Thermochemistry |
Nutrition |
Thermodynamics
|
Classification of Vegetable Oils by Principal Component Analysis of FTIR Spectra David A. Rusak, Leah M. Brown, and Scott D. Martin
Comparing unknown samples of vegetable oils to known samples using FTIR and principal component analysis (PCA) and nearest means classification (NMC).
Rusak, David A.; Brown, Leah M.; Martin, Scott D. J. Chem. Educ. 2003, 80, 541.
IR Spectroscopy |
Instrumental Methods |
Food Science |
Lipids |
Chemometrics |
Qualitative Analysis |
Fourier Transform Techniques |
Consumer Chemistry |
Applications of Chemistry
|
Incomplete Combustion with Candle Flames: A Guided-Inquiry Experiment in the First-Year Chemistry Lab Joseph MacNeil and Lisa Volaric
Investigating a burning candle as an introduction to incomplete combustion, thermodynamics, kinetics, and gas chromatography.
MacNeil, Joseph; Volaric, Lisa. J. Chem. Educ. 2003, 80, 302.
Chromatography |
Gases |
Reactions |
Oxidation / Reduction |
Thermodynamics |
Kinetics |
Gas Chromatography
|
Teaching Chemistry Using From the Earth to the Moon James G. Goll and Stacie L. Mundinger
Teaching chemistry using From the Earth to the Moon (an HBO original movie series).
Goll, James G.; Mundinger, Stacie L. J. Chem. Educ. 2003, 80, 292.
Electrochemistry |
Chemometrics |
Reactions |
Mechanisms of Reactions |
Applications of Chemistry
|
"Disorder" in Unstretched Rubber Bands? Warren Hirsch
Analysis of the thermodynamics of a stretched rubber band.
Hirsch, Warren. J. Chem. Educ. 2003, 80, 145.
Noncovalent Interactions |
Thermodynamics
|
"Disorder" in Unstretched Rubber Bands? Frank L. Lambert
Analysis of the thermodynamics of a stretched rubber band.
Lambert, Frank L. J. Chem. Educ. 2003, 80, 145.
Noncovalent Interactions |
Thermodynamics
|
"Disorder" in Unstretched Rubber Bands? Frank L. Lambert
Analysis of the thermodynamics of a stretched rubber band.
Lambert, Frank L. J. Chem. Educ. 2003, 80, 145.
Noncovalent Interactions |
Thermodynamics
|
Rubber Bands, Free Energy, and Le Châtelier's Principle Warren Hirsch
Using a rubber band to illustrate Gibbs free energy, entropy, and enthalpy.
Hirsch, Warren. J. Chem. Educ. 2002, 79, 200A.
Noncovalent Interactions |
Thermodynamics |
Equilibrium
|
Energy as Money, Chemical Bonding as Business, and Negative ΔH and ΔG as Investment Evguenii I. Kozliak
Analogy for explaining the sign (+ or -) of ?H, ?G, and ?S to introductory students.
Kozliak, Evguenii I. J. Chem. Educ. 2002, 79, 1435.
Nonmajor Courses |
Thermodynamics
|
Entropy Is Simple, Qualitatively Frank L. Lambert
Explanation of entropy in terms of energy dispersal; includes considerations of fusion and vaporization, expanding gasses and mixing fluids, colligative properties, and the Gibbs function.
Lambert, Frank L. J. Chem. Educ. 2002, 79, 1241.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Gases
|
An Interactive Graphical Approach to Temperature Conversions Jonathan Mitschele
Activity to demonstrate the relationship between the Fahrenheit and Celsius temperature scales by graphing measurements of English- and metric-unit thermometers.
Mitschele, Jonathan. J. Chem. Educ. 2002, 79, 1235.
Nomenclature / Units / Symbols |
Chemometrics |
Calorimetry / Thermochemistry
|
LIMSport: Optimizing a Windows-Based Computer Data Acquisition and Reduction System for the General Chemistry Laboratory Ed Vitz and Brenda P. Egolf
Project to develop a Windows/Excel data acquisition system for LIMSport (a mechanism for automatically acquiring data from a variety of sensors into a spreadsheet so that teachers and students only need spreadsheet skills to acquire and analyze data) and evaluate its effectiveness in promoting student learning.
Vitz, Ed; Egolf, Brenda P. J. Chem. Educ. 2002, 79, 1060.
Laboratory Computing / Interfacing |
Learning Theories |
Chemometrics
|
Precision in Microscale Titration Mono M. Singh, Cynthia B. McGowan, and Zvi Szafran
Comparing the precision of a 2-mL graduated pipet and 50-mL graduated buret in performing a microscale titration.
Singh, Mono M.; McGowan, Cynthia B.; Szafran, Zvi. J. Chem. Educ. 2002, 79, 941.
Laboratory Equipment / Apparatus |
Chemometrics |
Microscale Lab |
Titration / Volumetric Analysis
|
Precision in Microscale Titration Julian L. Roberts Jr.
Comparing the precision of a 2-mL graduated pipet and 50-mL graduated buret in performing a microscale titration.
Roberts, Julian L., Jr. J. Chem. Educ. 2002, 79, 941.
Laboratory Equipment / Apparatus |
Chemometrics |
Microscale Lab |
Titration / Volumetric Analysis
|
Precision in Microscale Titration Julian L. Roberts Jr.
Comparing the precision of a 2-mL graduated pipet and 50-mL graduated buret in performing a microscale titration.
Roberts, Julian L., Jr. J. Chem. Educ. 2002, 79, 941.
Laboratory Equipment / Apparatus |
Chemometrics |
Microscale Lab |
Titration / Volumetric Analysis
|
Understanding of Elementary Concepts in Heat and Temperature among College Students and K–12 Teachers Paul G. Jasien and Graham E. Oberem
Report on a study of the understanding of elementary concepts related to heat and temperature (thermal equilibrium and energy transfer in the form of heat) in undergraduate and post-baccalaurate students as a function of their number of semesters of college-level physical science training.
Jasien, Paul G.; Oberem, Graham E. J. Chem. Educ. 2002, 79, 889.
Thermodynamics |
Equilibrium
|
Experimental Design and Multiplexed Modeling Using Titrimetry and Spreadsheets Peter de B. Harrington, Erin Kolbrich, and Jennifer Cline
Determining the acidity of three vinegar samples using multiplexed titrations and an MS Excel spreadsheet.
Harrington, Peter de B.; Kolbrich, Erin; Cline, Jennifer. J. Chem. Educ. 2002, 79, 863.
Acids / Bases |
Chemometrics |
Stoichiometry |
Titration / Volumetric Analysis
|
H Is for Enthalpy, Thanks to Heike Kamerlingh Onnes and Alfred W. Porter Irmgard K. Howard
Origin of the word enthalpy.
Howard, Irmgard K. J. Chem. Educ. 2002, 79, 697.
Thermodynamics |
Calorimetry / Thermochemistry
|
A Chemically Relevant Model for Teaching the Second Law of Thermodynamics Bryce E. Williamson and Tetsuo Morikawa
Presentation of a chemically relevant model that exemplifies many aspects of the second law: reversibility, path dependence, and extrapolation in terms of electrochemistry and calorimetry.
Williamson, Bryce E.; Morikawa, Tetsuo. J. Chem. Educ. 2002, 79, 339.
Calorimetry / Thermochemistry |
Electrochemistry |
Thermodynamics
|
The Lead-Acid Battery: Its Voltage in Theory and in Practice Richard S. Treptow
Lead-acid battery fundamentals, cell voltage and the Nernst equation, and an analysis of actual battery performance.
Treptow, Richard S. J. Chem. Educ. 2002, 79, 334.
Electrochemistry |
Oxidation / Reduction |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials |
Acids / Bases |
Applications of Chemistry
|
Nonlinear Fits of Standard Curves: A Simple Route to Uncertainties in Unknowns Carl Salter and Robert de Levie
The problem of covariance in using calibration curves and a nonlinear least-squares procedure that permits a direct estimation of uncertainty without the need for covariance.
Salter, Carl; de Levie, Robert. J. Chem. Educ. 2002, 79, 268.
Chemometrics
|
Spontaneous Assembly of Soda Straws D. J. Campbell, E. R. Freidinger, J. M. Hastings, and M. K. Querns
Demonstrating spontaneous assembly using soda straws.
Campbell, D. J.; Freidinger, E. R.; Hastings, J. M.; Querns, M. K. J. Chem. Educ. 2002, 79, 201.
Materials Science |
Molecular Properties / Structure |
Nanotechnology |
Surface Science |
Thermodynamics
|
Disorder--A Cracked Crutch for Supporting Entropy Discussions Frank L. Lambert
Arguments against using disorder as a means of introducing and teaching entropy.
Lambert, Frank L. J. Chem. Educ. 2002, 79, 187.
Thermodynamics
|
Some Unusual Applications of the "Error-Bar" Feature in Excel Spreadsheets Kieran F. Lim
Paper demonstrating how the "error-bar" feature in Excel can be sued to produce high-quality graphs for university teaching, learning, and research.
Lim, Kieran F. J. Chem. Educ. 2002, 79, 135.
Chemometrics
|
Visualizing the Photochemical Steady State with UV-Sensitive Beads (re J. Chem. Educ. 2001, 77, 648A-648B) Jerry A. Bell
Analysis of the temperature dependence of the color intensity of UV-sensitive beads.
Bell, Jerry A. J. Chem. Educ. 2001, 78, 1594.
Atomic Properties / Structure |
Kinetics |
Photochemistry |
Chemometrics
|
On Concepts of Partial Volume and Law of Partial Volume (re J. Chem. Educ. 2001, 78, 238-240) Myung-Hoon Kim
Supplementing the law of partial pressures with a law of partial volumes.
Kim, Myung-Hoon. J. Chem. Educ. 2001, 78, 1594.
Gases |
Chemometrics |
Physical Properties
|
On Concepts of Partial Volume and Law of Partial Volume (re J. Chem. Educ. 2001, 78, 238-240) David W. Miller
Supplementing the law of partial pressures with a law of partial volumes.
Miller, David W. J. Chem. Educ. 2001, 78, 1594.
Gases |
Chemometrics |
Physical Properties
|
On the Importance of Ideality Rubin Battino, Scott E. Wood, and Arthur G. Williamson
Analysis of the utility of ideality in gaseous phenomena, solutions, and the thermodynamic concept of reversibility.
Battino, Rubin; Wood, Scott E.; Williamson, Arthur G. J. Chem. Educ. 2001, 78, 1364.
Thermodynamics |
Gases |
Solutions / Solvents
|
Experiencing and Visualizing the First Law of Thermodynamics: An In-Class Workshop Pamela Mills, William V. Sweeney, and Waldemar Cieniewicz
A handheld device that illustrates the concepts of heat, work, energy transfer, and thermodynamic path.
Mills, Pamela; Sweeney, William V.; Cieniewicz, Waldemar. J. Chem. Educ. 2001, 78, 1360.
Gases |
Thermodynamics |
Laboratory Equipment / Apparatus |
Laboratory Computing / Interfacing
|
Analysis of Success in General Chemistry Based on Diagnostic Testing Using Logistic Regression Margaret J. Legg, Jason C. Legg, and Thomas J. Greenbowe
Estimating the probability of succeeding in general chemistry based on diagnostic or placement exam scores.
Legg, Margaret J.; Legg, Jason C.; Greenbowe, Thomas J. J. Chem. Educ. 2001, 78, 1117.
Chemometrics |
Learning Theories |
Student / Career Counseling
|
A Simplified Method for Measuring the Entropy Change of Urea Dissolution. An Experiment for the Introductory Chemistry Lab Charles A. Liberko and Stephanie Terry
Guided inquiry to determine values for changes in enthalpy, Gibb's free energy, and entropy for the dissolution of urea in water.
Liberko, Charles A.; Terry, Stephanie. J. Chem. Educ. 2001, 78, 1087.
Thermodynamics |
Calorimetry / Thermochemistry
|
The Isothermal Heat Conduction Calorimeter: A Versatile Instrument for Studying Processes in Physics, Chemistry, and Biology Lars Wadsö, Allan L. Smith, Hamid Shirazi, S. Rose Mulligan, and Thomas Hofelich
A simple but sensitive isothermal heat-conduction calorimeter and five experiments for students to illustrate its use (heat capacity of solids, acid-base titration, enthalpy of vaporization of solvents, cement hydration, and insect metabolism).
Wadsö, Lars; Smith, Allan L.; Shirazi, Hamid; Mulligan, S. Rose; Hofelich, Thomas. J. Chem. Educ. 2001, 78, 1080.
Calorimetry / Thermochemistry |
Laboratory Equipment / Apparatus |
Thermal Analysis |
Thermodynamics
|
Stories to Make Thermodynamics and Related Subjects More Palatable Lawrence S. Bartell
Collection of anecdotes regarding the history and human side of chemistry.
Bartell, Lawrence S. J. Chem. Educ. 2001, 78, 1059.
Surface Science |
Thermodynamics |
Kinetic-Molecular Theory |
Applications of Chemistry
|
Melting Point, Density, and Reactivity of Metals Michael Laing
Using melting points and densities to the predict the relative reactivities of metals.
Laing, Michael. J. Chem. Educ. 2001, 78, 1054.
Descriptive Chemistry |
Metals |
Periodicity / Periodic Table |
Physical Properties |
Reactions |
Thermodynamics |
Calorimetry / Thermochemistry |
Electrochemistry
|
Don't Be Tricked by Your Integrated Rate Plot! Edward T. Urbansky
Using integrated rate plots to determine reaction order.
Urbansky, Edward T. J. Chem. Educ. 2001, 78, 921.
Kinetics |
Mechanisms of Reactions |
Learning Theories |
Chemometrics |
Rate Law
|
An Alcohol Rocket Car--A Variation on the "Whoosh Bottle" Theme Dean J. Campbell
Burning methanol in a wheeled milk jug.
Campbell, Dean J. J. Chem. Educ. 2001, 78, 910.
Gases |
Thermodynamics
|
A Simple Computer-Interfaced Calorimeter: Application to the Determination of the Heat of Formation of Magnesium Oxide Sze-Shun Wong, Natasha D. Popovich, and Shelley J. Coldiron
Design, construction, and laboratory instructional application of a simple computer-controlled, constant-pressure calorimeter.
Wong, Sze-Shun; Popovich, Natasha D.; Coldiron, Shelley J. J. Chem. Educ. 2001, 78, 798.
Calorimetry / Thermochemistry |
Instrumental Methods |
Thermodynamics |
Laboratory Equipment / Apparatus
|
A Simple Method for Illustrating Uncertainty Analysis Paul C. Yates
A fast and simple method for generating data for uncertainty analysis; includes statistical analysis and calculation of maximum probable error for a sample set of data.
Yates, Paul C. J. Chem. Educ. 2001, 78, 770.
Chemometrics |
Quantitative Analysis
|
Chemistry Report. MAA-CUPM Curriculum Foundations Workshop in Biology and Chemistry, Macalester College, November 2-5, 2000 Norman C. Craig
Chemists list specific knowledge and skills in mathematics needed by chemistry students and indicate whether mathematicians or chemists should deliver the instruction; the course level of the instruction and the use of technological aids are also designated.
Craig, Norman C. J. Chem. Educ. 2001, 78, 582.
Chemometrics |
Mathematics / Symbolic Mathematics |
Learning Theories
|
What's Been Happening to Undergraduate Mathematics David M. Bressoud
An overview of some of the changes that have been occurring in undergraduate mathematics education; based on a workshop held by the Mathematical Association of America to determine what chemists expect their students to learn from undergraduate mathematics courses in terms of understanding, content, and use of technology.
Bressoud, David M. J. Chem. Educ. 2001, 78, 578.
Learning Theories |
Mathematics / Symbolic Mathematics |
Chemometrics
|
Understanding Solubility through Excel Spreadsheets Pamela Brown
This article describes assignments related to the solubility of inorganic salts that can be given in an introductory general chemistry course. These assignments address the need for math, graphing, and computer skills in the chemical technology program by developing skill in the use of Microsoft Excel to prepare spreadsheets and graphs and to perform linear and nonlinear curve-fitting.
Brown, Pamela. J. Chem. Educ. 2001, 78, 268.
Aqueous Solution Chemistry |
Chemometrics |
Precipitation / Solubility
|
A Simple Laboratory Experiment for the Determination of Absolute Zero Myung-Hoon Kim, Michelle Song Kim, and Suw-Young Ly
A novel method that employs a remarkably simple and inexpensive apparatus and is based on the extrapolation of the volume of a given amount of dry air to zero volume after a volume of air trapped inside a 10-mL graduated cylinder is measured at various temperatures.
Kim, Myung-Hoon; Kim, Michelle Song; Ly, Suw-Young. J. Chem. Educ. 2001, 78, 238.
Gases |
Physical Properties |
Chemometrics
|
How Can an Instructor Best Introduce the Topic of Significant Figures to Students Unfamiliar with the Concept? Richard A. Pacer
The focus of this paper is how best to introduce the concept of significant figures so that students find it meaningful before a stage is reached at which they become turned off. The approach described begins with measurements students are already familiar with from their life experiences and involves the students as active learners.
Pacer, Richard A. J. Chem. Educ. 2000, 77, 1435.
Learning Theories |
Nonmajor Courses |
Chemometrics
|
Interpretation of Second Virial Coefficient Vivek Utgikar
Identifying the gel point of a polymer using a multimeter.
Utgikar, Vivek. J. Chem. Educ. 2000, 77, 1409.
Kinetics |
Lasers |
Spectroscopy |
Gases |
Thermodynamics
|
Thermodynamics of Water Superheated in the Microwave Oven B. H. Erné
Water is conveniently heated above its normal boiling point in a microwave oven in a glass microwave oven teapot. Water stops boiling soon after heating is interrupted, but subsequently added rough particles can still act as nucleation centers for a brief, spectacular burst of steam bubbles. The heat to make those steam bubbles obviously comes from the water itself, so that one can conclude that the boiling water was superheated, which is confirmed with a thermometer.
Erné, B. H. J. Chem. Educ. 2000, 77, 1309.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Water / Water Chemistry |
Liquids
|
Hell May Be Hotter Than Heaven After All (about J. Chem. Educ. 1999, 76, 503) M. N. Berberan-Santos
Estimation of temperatures in heaven and hell based on biblical information.
Berberan-Santos, Mário N. J. Chem. Educ. 2000, 77, 1278.
Nonmajor Courses |
Calorimetry / Thermochemistry |
Thermodynamics
|
Ernest Rutherford, Avogadro's Number, and Chemical Kinetics Revisited (about J. Chem. Educ. 1998, 75, 998-1003) James E. Sturm
Estimation of temperatures in heaven and hell based on biblical information.
Sturm, James E. J. Chem. Educ. 2000, 77, 1278.
Nonmajor Courses |
Calorimetry / Thermochemistry |
Thermodynamics |
Atomic Properties / Structure |
Kinetics |
Nuclear / Radiochemistry
|
Pixel Conversion: A Simple Way to Extract Coordinates of Points from a Printed Graph Christian Aymard and Randall B. Shirts
A very simple method is described for extracting the coordinates of points from printed graphs, student reports, or publications. One only needs a flatbed scanner and a desktop computer. This is a convenient and inexpensive alternative to the tedious traditional method using a ruler or to the more costly programs available commercially. A Windows program has been made available to perform the required operations.
Aymard, Christian; Shirts, Randall B. J. Chem. Educ. 2000, 77, 1230.
Chemometrics
|
A Visual Aid in Enthalpy Calculations Sebastian G. Canagaratna
This article discusses the use of enthalpy-temperature diagrams for reactants and products as a visual aid in the teaching of reaction-enthalpy calculations. By the use of such diagrams the division of the process into a part involving a chemical reaction without a temperature change and a part involving only a temperature change is made visually concrete.
Canagaratna, Sebastian G. J. Chem. Educ. 2000, 77, 1178.
Thermodynamics |
Calorimetry / Thermochemistry
|
Encouraging Meaningful Quantitative Problem Solving Jeff Cohen, Meghan Kennedy-Justice, Sunny Pai, Carmen Torres, Rick Toomey, Ed DePierro, and Fred Garafalo
This paper describes the efforts of a group of teachers to help college freshman chemistry students and high school science students to improve their problem-solving skills. The presentation includes several sets of questions intended to elucidate ideas and to involve the reader in the process of reflecting upon his or her own problem-solving strategies.
Cohen, Jeff; Kennedy-Justice, Meghan; Pai, Sunny; Torres, Carmen; Toomey, Rick; DePierro, Ed; Garafalo, Fred. J. Chem. Educ. 2000, 77, 1166.
Mathematics / Symbolic Mathematics |
Chemometrics
|
Determination of Ksp, ΔG0, ΔH0, and ΔS0 for the Dissolution of Calcium Hydroxide in Water: A General Chemistry Experiment William B. Euler, Louis J. Kirschenbaum, and Ben Ruekberg
This exercise utilizes low-cost, relatively nonhazardous materials presenting few disposal problems. It reinforces the students' understanding of the interrelationship of solubility, Ksp, ΔG0, ΔH0, and ΔS0.
Euler, William B.; Kirschenbaum, Louis J.; Ruekberg, Ben. J. Chem. Educ. 2000, 77, 1039.
Equilibrium |
Thermodynamics |
Titration / Volumetric Analysis
|
Understanding Electrochemical Thermodynamics through Entropy Analysis Thomas H. Bindel
This discovery-based activity involves entropy analysis of galvanic cells. The intent of the activity is for students to discover the fundamentals of electrochemical cells through a combination of entropy analysis, exploration, and guided discovery.
Bindel, Thomas H. J. Chem. Educ. 2000, 77, 1031.
Electrochemistry |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials
|
A Classroom Exercise in Sampling Technique Michael R. Ross
A classroom hands-on demonstration has been developed that looks at the two important sampling considerations, sample size and non-homogeneous sample materials. This classroom activity makes use of readily available M&M candies for the sample size and NERDS for the non-homogeneous sample exercises.
Ross, Michael R. J. Chem. Educ. 2000, 77, 1015.
Quantitative Analysis |
Chemometrics
|
A Closer Look at Phase Diagrams for the General Chemistry Course Stephen A. Gramsch
The information provided by the high-pressure phase diagrams of some simple systems (carbon dioxide, water, hydrogen, and iron) can provide a useful extension to the traditional discussion of phase diagrams in the general chemistry course. At the same time, it can prepare students for a more illuminating presentation of the concept of equilibrium than is possible through the discussion of gas phase, acid-base, and solubility product equilibria alone.
Gramsch, Stephen A. J. Chem. Educ. 2000, 77, 718.
Equilibrium |
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Geochemistry
|
Ionic Crystals: A Simple and Safe Lecture Demonstration of the Preparation of NaI from Its Elements Zelek S. Herman
A simple and safe classroom demonstration showing the production of sodium iodide (NaI) crystals from elemental sodium and elemental (molecular) iodine is presented. The demonstration, which is quite impressive, naturally fits into the discussion of ionic bonding and the alkali halide crystals.
Herman, Zelek S. J. Chem. Educ. 2000, 77, 619.
Crystals / Crystallography |
Thermodynamics |
Ionic Bonding |
Crystals / Crystallography
|
Illustrating Thermodynamic Concepts Using a Hero's Engine Pedro L. Muiño and James R. Hodgson
A modified Hero's engine is used to illustrate concepts of thermodynamics and engineering design suitable for introductory chemistry courses and more advanced physical chemistry courses. This demonstration is suitable to illustrate concepts like gas expansion, gas cooling through expansion, conversion of heat to work, interconversion between kinetic energy and potential energy, and feedback mechanisms.
Muio, Pedro L.; Hodgson, James R. J. Chem. Educ. 2000, 77, 615.
Gases |
Thermodynamics |
Phases / Phase Transitions / Diagrams
|
Spreadsheet Calculation of the Propagation of Experimental Imprecision Robert de Levie
A spreadsheet is used to compute the propagation of imprecision, and a macro is described that will do this automatically.
de Levie, Robert. J. Chem. Educ. 2000, 77, 534.
Chemometrics |
Quantitative Analysis |
Laboratory Computing / Interfacing
|
The Use of Extent of Reaction in Introductory Courses Sebastian G. Canagaratna
This article discusses the use of the extent of reaction as an alternative to the traditional approach to stoichiometry in first-year chemistry. The method focuses attention on the reaction as a whole rather than on pairs of reagents as in the traditional approach. The balanced equation is used as the unit of change.
Canagaratna, Sebastian G. J. Chem. Educ. 2000, 77, 52.
Stoichiometry |
Thermodynamics |
Nomenclature / Units / Symbols
|
Boerhaave on Fire Damon Diemente
This article offers a selection of passages from Boerhaave's chapter on fire. Boerhaave offers demonstrations and experiments that can be instructively performed today, quantitative data that can be checked against modern equations, and much theory and hypothesis that can be assessed in light of modern chemical ideas.
Diemente, Damon. J. Chem. Educ. 2000, 77, 42.
Calorimetry / Thermochemistry |
Thermodynamics
|
Using TOPEX Satellite El Niño Altimetry Data to Introduce Thermal Expansion and Heat Capacity Concepts in Chemistry Courses Harvey F. Blanck
Warm water is less dense than cool water and will float somewhat like ice, with a portion above the surface of the cooler surrounding water. The height of the bump can be used to estimate the excess thermal energy in the warmer water.
Blanck, Harvey F. J. Chem. Educ. 1999, 76, 1635.
Liquids |
Thermodynamics |
Water / Water Chemistry |
Calorimetry / Thermochemistry
|
Entropy, Disorder, and Freezing Brian B. Laird
It is argued that the usual view that entropy is a measure of "disorder" is problematic and that there exist systems at high density, for which packing considerations dominate, where a spatially ordered state has a higher entropy than a disordered one.
Laird, Brian B. J. Chem. Educ. 1999, 76, 1388.
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Statistical Mechanics
|
Shuffled Cards, Messy Desks, and Disorderly Dorm Rooms - Examples of Entropy Increase? Nonsense! Frank L. Lambert
Simply changing the location of everyday macro objects from an arrangement that we commonly judge as orderly to one that appears disorderly is a "zero change" in the thermodynamic entropy of the objects because the number of accessible energetic microstates in any of them has not been changed.
Lambert, Frank L. J. Chem. Educ. 1999, 76, 1385.
Nonmajor Courses |
Statistical Mechanics |
Thermodynamics
|
Visualizing Entropy Joseph H. Lechner
This report describes two classroom activities that help students visualize the abstract concept of entropy and apply the second law of thermodynamics to real situations.
Lechner, Joseph H. J. Chem. Educ. 1999, 76, 1382.
Statistical Mechanics |
Thermodynamics
|
Chemistry Comes Alive! Vol. 3: Abstract of Special Issue 23 on CD-ROM Jerrold J. Jacobsen and John W. Moore
Volume 3 contains several related topics generally included in an introductory chemistry course. The general areas are Enthalpy and Thermodynamics, Oxidation-Reduction, and Electrochemistry.
Jacobsen, Jerrold J.; Moore, John W. J. Chem. Educ. 1999, 76, 1311.
Calorimetry / Thermochemistry |
Thermodynamics |
Oxidation / Reduction |
Electrochemistry
|
Predicting Acid-Base Titration Curves without Calculations Dennis W. Barnum
In this paper a qualitative and systematic method for sketching titration curves is presented. Even the more complex cases such as salts or polyprotic acids and bases are treated just as easily as simple monoprotic acids. Having students predict the shape of titration curves from known equilibrium constants helps to focus attention on the general principles without distraction by the mathematics.
Barnum, Dennis W. J. Chem. Educ. 1999, 76, 938.
Acids / Bases |
Quantitative Analysis |
Water / Water Chemistry |
Equilibrium |
Learning Theories |
Titration / Volumetric Analysis |
Chemometrics
|
Do pH in Your Head Addison Ault
Every aqueous solution has a pH. Two factors determine this pH: the acidic or basic strength of the solute, and its concentration. When you use pKa values to express acidic and basic strength you can easily estimate the approximate pH of many aqueous solutions of acids, bases, and their salts and their buffers.
Ault, Addison. J. Chem. Educ. 1999, 76, 936.
Equilibrium |
Acids / Bases |
Aqueous Solution Chemistry |
Learning Theories |
Chemometrics |
Brønsted-Lowry Acids / Bases
|
The Evolution of the Celsius and Kelvin Temperature Scales and the State of the Art Julio Pellicer, M. Amparo Gilabert, and Ernesto Lopez-Baeza
A physical analysis is given of the evolution undergone by the Celsius and Kelvin temperature scales, from their definition to the present day.
Pellicer, Julio; Gilabert, M. Amparo; Lopez-Baeza, Ernesto. J. Chem. Educ. 1999, 76, 911.
Nomenclature / Units / Symbols |
Thermodynamics |
Learning Theories
|
Precision and Accuracy in Measurements (the author replies) Treptow, Richard S.
Relation between instrument resolution and skill.
Treptow, Richard S. J. Chem. Educ. 1999, 76, 471.
Chemometrics |
Instrumental Methods
|
Precision and Accuracy in Measurements Thomsen, Volker
The difference between instrument resolution and precision.
Thomsen, Volker J. Chem. Educ. 1999, 76, 471.
Chemometrics |
Instrumental Methods
|
An Easy and Effective Classroom Demonstration of Population Distributions Marjorie A. Jones
Using a simple experimental design and easily obtained materials, a classroom experiment was conducted to demonstrate normal-distribution behavior for a population. We used popcorn and a hot-air popper. Popped kernels were collected with time and data were plotted as popped kernels per time interval versus time. The data clearly showed a normal (Gaussian) distribution.
Jones, Marjorie A. J. Chem. Educ. 1999, 76, 384.
Chemometrics
|
The Ammonia Smoke Fountain: An Interesting Thermodynamic Adventure M. Dale Alexander
The ammonia smoke fountain demonstration utilizes a modification of the apparatus used in the standard ammonia fountain. The modification allows for the introduction of hydrogen chloride gas into a flask of ammonia rather than water. The flow rate of hydrogen chloride gas into the flask in the smoke fountain is not constant, but periodic; that is, the smoke puffs from the end of the tube. This unexpected behavior elicits an interesting thermodynamic explanation.
Alexander, M. Dale. J. Chem. Educ. 1999, 76, 210.
Acids / Bases |
Gases |
Thermodynamics |
Reactions |
Stoichiometry |
Precipitation / Solubility
|
Effect of Sample Size on Sampling Error: An Experiment for Introductory Analytical Chemistry Joseph E. Vitt and Royce C. Engstrom
Students acquire samples of various size from a binary population, calculate the relative standard deviations for each sample size, and compare these results with those predicted by the binomial distribution. This experiment gives excellent agreement for the pooled student data, and the results show the expected decrease in sampling error as the sample size increases.
Vitt, Joseph E.; Engstrom, Royce C. J. Chem. Educ. 1999, 76, 99.
Quantitative Analysis |
Instrumental Methods |
Chemometrics
|
CHEMiCALC (4000161) and CHEMiCALC Personal Tutor (4001108), Version 4.0 (by O. Bertrand Ramsay) Scott White and George Bodner
CHEMiCALC is a thoughtfully designed software package developed for use by high school and general chemistry students, who will benefit from the personal tutor mode that helps to guide them through unit conversion, empirical formula, molecular weight, reaction stoichiometry, and solution stoichiometry calculations.
White, Scott; Bodner, George M. J. Chem. Educ. 1999, 76, 34.
Chemometrics |
Nomenclature / Units / Symbols |
Stoichiometry
|
Temperature Scale Conversion as a Linear Equation: True Unit Conversion vs Zero-Offset Correction Reuben Rudman
The equation used for the interconversion between the Fahrenheit and Celsius temperature scales is in reality the general case of the straight-line equation (y = ax + b). This equation is the paradigm for many of the calculations taught in introductory chemistry.
Rudman, Reuben. J. Chem. Educ. 1998, 75, 1646.
Nomenclature / Units / Symbols |
Chemometrics
|
Modeling Nuclear Decay: A Point of Integration between Chemistry and Mathematics Kent J. Crippen and Robert D. Curtright
A four-part activity utilizing a graphing calculator to investigate nuclear stability is described. Knowledge acquired through the activity provides background for answering the societal question of using nuclear materials for energy production.
Crippen, Kent J.; Curtright, Robert D. J. Chem. Educ. 1998, 75, 1434.
Nuclear / Radiochemistry |
Atomic Properties / Structure |
Chemometrics
|
There Seems To Be Uncertainty about the Use of Significant Figures in Reporting Uncertainties of Results Julio F. Caballero and Delphia F. Harris
A cursory review of two journals indicates that uncertainties in experimental results are not consistently reported in the literature with the correct number of significant figures. The problem seems more frequent in computer generated results in both chemical education and research articles. Examples of published values with uncertainty inappropriately reported are included along with the appropriate rounding.
Caballero, Julio F.; Harris, Delphia F. J. Chem. Educ. 1998, 75, 996.
Laboratory Equipment / Apparatus |
Learning Theories |
Chemometrics
|
Precision and Accuracy in Measurements: A Tale of Four Graduated Cylinders Richard S. Treptow
The concepts of precision and accuracy help students understand that uncertainty accompanies even our best scientific measurements. A model experiment can be used to distinguish the two terms. The experiment uses four graduated cylinders which give measurements of different accuracy and precision. Such terms as mean, range, standard deviation, error, and true value are defined through an illustration.
Treptow, Richard S. J. Chem. Educ. 1998, 75, 992.
Quantitative Analysis |
Chemometrics
|
Precision and Accuracy (the authors reply, 2) Midden, W. Robert
Rounding-off rules and significant figures.
Midden, W. Robert J. Chem. Educ. 1998, 75, 971.
Chemometrics
|
Precision and Accuracy (the authors reply, 1) Guare, Charles J.
Rounding-off rules and significant figures.
Guare, Charles J. J. Chem. Educ. 1998, 75, 971.
Chemometrics
|
Precision and Accuracy (3) Rustad, Douglas
Rounding-off rules and significant figures.
Rustad, Douglas J. Chem. Educ. 1998, 75, 970.
Chemometrics
|
Precision and Accuracy (1) Sykes, Robert M.
Standard procedures for determining and maintaining significant figures in calculations.
Sykes, Robert M. J. Chem. Educ. 1998, 75, 970.
Chemometrics
|
Percent Composition and Empirical Formula - A New View George L. Gilbert
A new method of obtaining the empirical formula for a compound from its percent composition is proposed. The method involves the determination of a minimum molar mass for the compound based on the percentage of each element, obtaining the lowest common molar mass and using this data to calculate the integer values used in writing the empirical formula.
Gilbert, George L. J. Chem. Educ. 1998, 75, 851.
Atomic Properties / Structure |
Stoichiometry |
Chemometrics
|
Vapor Pressure Lowering by Nonvolatile Solutes Gavin D. Peckham
This short article highlights a fundamental error that is entrenched in introductory chemistry textbooks. It is true that the addition of a nonvolatile solute causes a lowering in the vapor pressure of a solution. The error lies in attributing this vapor pressure lowering to the "blocking" of surface sites by nonvolatile particles. This is a totally fallacious argument for a number of reasons and the true explanation is to be found in the entropy changes that occur as a nonvolatile solute is added to a solution.
Peckham, Gavin D. J. Chem. Educ. 1998, 75, 787.
Gases |
Solutions / Solvents |
Thermodynamics
|
Sugar Dehydration without Sulfuric Acid: No More Choking Fumes in the Classroom! Todd P. Silverstein and Yi Zhang
Our demonstration uses no sulfuric acid, yields relatively little smoke, and produces an exciting and unpredictable growing column of black carbon.
Silverstein, Todd P.; Zhang, Yi. J. Chem. Educ. 1998, 75, 748.
Carbohydrates |
Thermodynamics |
Electrochemistry |
Solid State Chemistry |
Oxidation / Reduction
|
Thermodynamics and Spontaneity (the author replies) Ochs, Raymond S.
The term "spontaneous" is historical baggage.
Ochs, Raymond S. J. Chem. Educ. 1998, 75, 659.
Thermodynamics
|
Thermodynamics and Spontaneity Earl, Boyd L.
The term "spontaneous" is worth keeping in the chemistry lexicon.
Earl, Boyd L. J. Chem. Educ. 1998, 75, 658.
Thermodynamics
|
Letters to the Editor
The term "spontaneous" is worth keeping in the chemistry lexicon.
J. Chem. Educ. 1998, 75, 658.
Thermodynamics
|
Production of Numerical Chemical Problems Using a Spreadsheet Peter G. Hall
The use of spreadsheets for "personalized" assignments. These assignments take the form of printed chemical problems such that every student has different numerical data. The problem sets make a challenging student introduction to word processing and spreadsheet use.
Hall, Peter G. J. Chem. Educ. 1998, 75, 243.
Chemometrics
|
Demonstrating Heat Changes on the Overhead Projector with a Projecting Thermometer Chinhyu Hur, Sally Solomon, and Christy Wetzel
Heat changes can be observed by using a culture dish and a thermometer that is projected onto a screen using an overhead projector.
Hur, Chinhyu; Solomon, Sally; Wetzel, Christy. J. Chem. Educ. 1998, 75, 51.
Calorimetry / Thermochemistry |
Solutions / Solvents |
Thermodynamics |
Laboratory Equipment / Apparatus
|
Heat Capacity, Body Temperature, and Hypothermia Doris R. Kimbrough
A finger in and out of water are compared to demonstrate the difference between heat capacities and their effect on body temperature.
Kimbrough, Doris R. J. Chem. Educ. 1998, 75, 48.
Calorimetry / Thermochemistry |
Thermodynamics
|
The Chemistry Maths Book (by Erich Steiner) C. Michael McCallum
The Chemistry Maths Book contains all the mathematical methods that 99% of chemists would need. Designed as a text for an actual Maths for Chemists course, it is laid out in a logical progression from simple (decimals, algebra, and functions) to the more complicated but no less important (matrix algebra, differential equations, and matrix eigenvalue problems). It seems well suited both for its stated purpose and as a "brush-up" book for undergraduates, graduate students, and others.
McCallum, C. Michael. J. Chem. Educ. 1997, 74, 1400.
Chemometrics |
Mathematics / Symbolic Mathematics
|
A Note on Covariance in Propagation of Uncertainty Edwin F. Meyer
It is pointed out that whenever both the slope and the intercept are used in calculating a physical quantity from a linear regression, propagation of error must include the covariance as well as the variances. The point is illustrated with a calculation of the boiling point of water from the parameters of the lnP vs 1/T fit. If the covariance is omitted from the propagation of error, the estimate of uncertainty is unreasonably large.
Meyer, Edwin F. J. Chem. Educ. 1997, 74, 1339.
Chemometrics
|
Spreadsheet Applications in Chemistry Using Microsoft Excel by Dermot Diamond and Venita C. A. Hanratty Jeffery A. Greathouse
Provides chemistry instructors with an introduction to Excel and its applications in chemistry.
Greathouse, Jeffery A. J. Chem. Educ. 1997, 74, 1279.
Chemometrics
|
MathBrowser: Web-Enabled Mathematical Software with Application to the Chemistry Curriculum, v 1.0 Jack G. Goldsmith
MathBrowser, a freeware web-enabled derivative of the MathCad mathematical software (MathSoft Inc., Cambridge, MA), is designed to reconcile the problem of how to distribute mathematically rich information over the WWW and to maintain interactivity for the end user.
Goldsmith, Jack G. J. Chem. Educ. 1997, 74, 1164.
Mathematics / Symbolic Mathematics |
Chemometrics
|
Graham's Law and Perpetuation of Error Stephen J. Hawkes
Grahams Laws of effusion and diffusion are used in recent articles for traditional experiments to which they do not in fact apply and for which they give the wrong answer.
Hawkes, Stephen J. J. Chem. Educ. 1997, 74, 1069.
Gases |
Chemometrics |
Transport Properties
|
Why Don't Things Go Wrong More Often? Activation Energies: Maxwell's Angels, Obstacles to Murphy's Law Frank L. Lambert
The micro-complexity of fracturing utilitarian or beautiful objects prevents assigning a characteristic activation energy even to chemically identical artifacts. Nevertheless, a qualitative EACT SOLID can be developed. Its surmounting is correlated with the radical drop in human valuation of an object when it is broken.
Lambert, Frank L. J. Chem. Educ. 1997, 74, 947.
Kinetics |
Nonmajor Courses |
Thermodynamics
|
An Integrated-Circuit Temperature Sensor for Calorimetry and Differential Temperature Measurement Mark Muyskens
Application of an integrated-circuit (IC) temperature sensor which is easy-to-use, inexpensive, rugged, easily computer-interfacable and has good precision is described. The design, based on the National Semiconductor LM35 IC chip, avoids some of the difficulties associated with conventional sensors (thermocouples, thermistors, and platinum resistance thermometers) and a previously described IC sensor.
Muyskens, Mark. J. Chem. Educ. 1997, 74, 850.
Calorimetry / Thermochemistry |
Thermal Analysis |
Thermodynamics |
Laboratory Equipment / Apparatus |
Instrumental Methods
|
The Thermodynamics of Drunk Driving Robert Q. Thompson
Biological, chemical, and instrumental variables are described along with their contributions to the overall uncertainty in the value of BrAC/BAC.
Thompson, Robert Q. J. Chem. Educ. 1997, 74, 532.
Thermodynamics |
Nonmajor Courses |
Forensic Chemistry |
Drugs / Pharmaceuticals |
Applications of Chemistry
|
Rounding Numbers: Why the "New System" Doesn't Work W. Robert Midden
This paper explains a correction to the rounding rule previously published in this Journal. The earlier article reported that the best way to round numbers is to always round up when the first digit dropped is 5. However, this will lead to accumulation of error when errors are averaged.
Midden, W. Robert. J. Chem. Educ. 1997, 74, 405.
Chemometrics
|
Heat Flow vs. Cash Flow: A Banking Analogy Charles M. Wynn, Sr.
An analogy is drawn between the withdrawal of money from an automated teller machine (ATM) and an exothermic chemical reaction.
Wynn, Charles M. Sr. J. Chem. Educ. 1997, 74, 397.
Thermodynamics |
Calorimetry / Thermochemistry
|
Elasticity to Measure Thermodynamic Properties Jonathan Mitschele
Repetition of original experiment.
Mitschele, Jonathan. J. Chem. Educ. 1997, 74, 368.
Thermodynamics
|
Sensitivity to Experimental Parameters via Spreadsheets B. R. Sundheim
In spreadsheet computations wherever the functional dependence of calculated results on experimental quantities is obscure, sensitivities may be obtained by testing the effects of variations in relevant inputs. An example is given where Hess' law is explored calorimetrically.
Sundhein, B. R. . J. Chem. Educ. 1997, 74, 328.
Chemometrics
|
A Brief History of Thermodynamics Notation Rubin Battino, Laurence E. Strong, Scott E. Wood
This paper gives a brief history of thermodynamic notation for the energy, E, enthalpy, H, entropy, S, Gibbs energy, G, Helmholtz energy, A, work, W, heat, Q, pressure, P, volume, V, and temperature, T. In particular, the paper answers the question, "Where did the symbol S for entropy come from?"
Battino, Rubin; Strong Laurence E.; Wood, Scott E. J. Chem. Educ. 1997, 74, 304.
Thermodynamics
|
In Defense of Thermodynamics - An Animate Analogy Sture Nordholm
In order to illustrate the deepest roots of thermodynamics and its great power and generality, it is applied by way of analogy to human behavior from an economic point of view.
Nordholm, Sture. J. Chem. Educ. 1997, 74, 273.
Thermodynamics
|
Chemical Equilibrium (the author replies) Banerjee, Anil
Item 7 deserves a fuller answer than was provided.
Banerjee, Anil J. Chem. Educ. 1996, 73, A262.
Equilibrium |
Thermodynamics
|
Chemical Equilibrium Logan, S. R.
Item 7 deserves a fuller answer than was provided.
Logan, S. R. J. Chem. Educ. 1996, 73, A261.
Equilibrium |
Thermodynamics
|
Concept Maps in Chemistry Education Alberto Regis, Pier Giorgio Albertazzi, Ezio Roletto
This article presents and illustrates a proposed application of concept maps in chemistry teaching in high schools. Three examples of the use of concept maps in chemistry teaching are reported and discussed with reference to: atomic structure, oxidation-reduction and thermodynamics.
Regis, Alberto; Albertazzi, Pier Giorgio; Roletto, Ezio. J. Chem. Educ. 1996, 73, 1084.
Learning Theories |
Atomic Properties / Structure |
Oxidation / Reduction |
Thermodynamics
|
A Simple Method for Determining the Temperature Coefficient of Voltaic Cell Voltage Alfred E. Saieed, Keith M. Davies
This article describes a relatively simple method for preparing voltaic cells, and through their temperature coefficient, ?E/?T, it explores relationships between ?G, ?H,and ?S for the cell reactions involved.
Saieed, Alfred E.; Davies, Keith M. J. Chem. Educ. 1996, 73, 959.
Electrochemistry |
Calorimetry / Thermochemistry |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials |
Laboratory Equipment / Apparatus |
Laboratory Management |
Oxidation / Reduction
|
Thermodynamics and Spontaneity Raymond S. Ochs
Despite the importance of thermodynamics as the foundation of chemistry, most students emerge from introductory courses with only a dim understanding of this subject.
Ochs, Raymond S. J. Chem. Educ. 1996, 73, 952.
Thermodynamics |
Learning Theories |
Equilibrium
|
SIRS: Simulations and Interactive Resources, III Martin, John S.
Simulations and Interactive Resources (SIRs) are designed to support interactive lectures in introductory chemistry. This third issue of SIRs includes five new SIRs as well as updated and final versions of all previously published SIRs.
Martin, John S. J. Chem. Educ. 1996, 73, 722.
Periodicity / Periodic Table |
Equilibrium |
Gases |
Thermodynamics |
Reactions |
Electrochemistry |
Kinetics
|
An Approach to Reaction Thermodynamics through Enthalpies, Entropies, and Free Energies of Atomization James N. Spencer, Richard S. Moog, and Ronald J. Gillespie
An alternative to the conventional method of calculating enthalpies of reaction is presented, using enthalpies of atomization in place of enthalpies of formation. This allows the student to see directly that the reaction enthalpies are determined by the difference in bond strengths in the reactants and products.
James N. Spencer, Richard S. Moog, and Ronald J. Gillespie. J. Chem. Educ. 1996, 73, 631.
Calorimetry / Thermochemistry |
Thermodynamics |
Equilibrium |
Reactions |
Atomic Properties / Structure |
Stoichiometry
|
Solubility and Thermodynamics: An Introductory Experiment Robert G. Silberman
This article describes a laboratory experiment suitable for high school or freshman chemistry students in which the solubility of potassium nitrate is determined at several different temperatures.
Silberman, Robert G. J. Chem. Educ. 1996, 73, 426.
Precipitation / Solubility |
Thermodynamics |
Equilibrium
|
A Novel Approach to Teaching Electrochemical Principles Paul Krause and Jerry Manion
To demonstrate that work may be done by a chemical reaction, a reaction producing a gas is carried out in a large, closed syringe. As the gas is generated, the syringe plunger is forced out.
Krause, Paul; Manion, Jerry. J. Chem. Educ. 1996, 73, 354.
Reactions |
Gases |
Thermodynamics
|
Curve Fitting: An Alternative Approach to Analyzing Kinetic Data in Introductory Chemistry Coleman, William F.
183. The availability of high quality software for performing nonlinear curve fitting on microcomputers allows students to take an alternative approach to data analysis, one that concentrates on functional forms that may be more natural than some of the algebraic machinations necessary to render relationships into linear forms. An example of the application of such an approach to the analysis of kinetic data is presented in this paper.
Coleman, William F. J. Chem. Educ. 1996, 73, 243.
Chemometrics |
Kinetics
|
Significant Figures in Graph Interpretation Donald M. Graham
A means is derived for calculating the number of significant figures in the slope and intercept of an experimental linear graph. The method is based on the actual scatter in the points rather than on the nominal precision in the original data, and it can be used even by students who are mathematically fairly unsophisticated.
Graham, Donald M. J. Chem. Educ. 1996, 73, 211.
Chemometrics
|
Management of First-Year Chemistry Laboratories Using Spreadsheets Collins, Frank E.; Williams, Charles W.
Use of spreadsheets to record, analyze, and assess experimental data.
Collins, Frank E.; Williams, Charles W. J. Chem. Educ. 1995, 72, A182.
Chemometrics
|
Experimental Methods: An Introduction to the Analysis of Data (Kirkup, Les)
Title of interest.
J. Chem. Educ. 1995, 72, A72.
Chemometrics
|
Photosynthesis: Why Does It Occur? J. J. MacDonald
Explanation of why photosynthesis occurs; stating that it is merely the reverse of respiration is misleading.
MacDonald, J. J. J. Chem. Educ. 1995, 72, 1113.
Plant Chemistry |
Reactions |
Thermodynamics |
Photochemistry |
Electrochemistry
|
Dimensional Analysis: An Analogy to Help Students Relate the Concept to Problem Solving James R. McClure
Using dominoes to help students understand the conversion factor method of dimensional analysis.
McClure, James R. J. Chem. Educ. 1995, 72, 1093.
Nomenclature / Units / Symbols |
Chemometrics
|
Celsius to Fahrenheit--Quick and Dirty Colin Hester
Simple algorithm for converting Celsius temperature to Fahrenheit temperature.
Hester, Colin. J. Chem. Educ. 1995, 72, 1026.
Calorimetry / Thermochemistry |
Nomenclature / Units / Symbols |
Chemometrics
|
Determination of Heats of Fusion: Using Differential Scanning Calorimetry for the AP Chemistry Course Susan M. Temme
Using differential scanning calorimetry (DSC) in AP chemistry.
Temme, Susan M. J. Chem. Educ. 1995, 72, 916.
Calorimetry / Thermochemistry |
Calorimetry / Thermochemistry |
Physical Properties |
Phases / Phase Transitions / Diagrams |
Thermal Analysis |
Thermodynamics
|
Those Baffling Subscripts Arthur W. Friedel and David P. Maloney
Study of the difficulties students have in interpreting subscripts correctly and distinguishing atoms from molecules when answering questions and solving problems.
Friedel, Arthur W.; Maloney, David P. J. Chem. Educ. 1995, 72, 899.
Nomenclature / Units / Symbols |
Stoichiometry |
Chemometrics
|
How to Determine the Best Straight Line S. R. Logan
Consideration of situations in which the use of a least-squares regression is inappropriate.
Logan, S. R. J. Chem. Educ. 1995, 72, 896.
Chemometrics
|
The Relationship between the Number of Elements and the Number of Independent Equations of Elemental Balance in Inorganic Chemical Equations R. Subramanian, N.K. Goh, and L. S. Chia
The criterion for determining whether a chemical equation can be balanced fully by the algebraic technique and its application.
Subramaniam, R.; Goh, N. K.; Chia, L. S. J. Chem. Educ. 1995, 72, 894.
Stoichiometry |
Chemometrics
|
Teaching Chemical Equilibrium and Thermodynamics in Undergraduate General Chemistry Classes Anil C. Banerjee
Discussion of the conceptual difficulties experienced by undergraduates when dealing with equilibrium and thermodynamics, along with teaching strategies for dealing with these difficulties.
Banerjee, Anil C. J. Chem. Educ. 1995, 72, 879.
Equilibrium |
Thermodynamics
|
Synthesis and Decomposition of Zinc Iodide: Model Reactions for Investigating Chemical Change in the Introductory Laboratory Stephen DeMeo
Procedure for synthesizing and then decomposing zinc iodide in introductory chemistry that offers advantages over traditional synthesis/decomposition species (e.g. copper sulfide and magnesium oxide).
DeMeo, Stephen. J. Chem. Educ. 1995, 72, 836.
Synthesis |
Thermodynamics |
Reactions
|
From Titration Data to Buffer Capacities: A Computer Experiment for the Chemistry Lab or Lecture Roy W. Clark, Gary D. White, Judith M. Bonicamp, and Exum D. Watts
Provides titration curve data that students can plot and analyze using spreadsheets to develop student understanding of pH, derivatives, buffer capacity, and the behavior of dilute buffers; includes sample graphs and analysis.
Clark, Roy W.; White, Gary D.; Bonicamp, Judith M.; Watts, Exum D. J. Chem. Educ. 1995, 72, 746.
Acids / Bases |
pH |
Titration / Volumetric Analysis |
Chemometrics
|
Statistical Analysis Experiment for the Freshman Chemistry Lab John C. Salzsieder
Procedure that provides sufficient data for statistical analysis by a freshman chemistry class.
Salzsieder, John C. J. Chem. Educ. 1995, 72, 623.
Chemometrics
|
Buoyancy Programs; Viscosity of Polymer Solutions; Precision of Calculated Values Bertrand, Gary L.
Software to simulate the determination of the density of solids; the preparation of polymer solutions and their time to flow through a viscometer; and a program to calculate the uncertainties of results given the input values.
Bertrand, Gary L. J. Chem. Educ. 1995, 72, 492.
Physical Properties |
Chemometrics
|
Rapid Calculation for Preparing Solutions Calero, Diego Lozano
Streamlined method for dilution calculations.
Calero, Diego Lozano J. Chem. Educ. 1995, 72, 424.
Aqueous Solution Chemistry |
Solutions / Solvents |
Chemometrics
|
The MATCH Program: A Combined Mathematics and Chemistry Curriculum Wink, Donald J.
A curriculum that integrates introductory chemistry with intermediate algebra.
Wink, Donald J. J. Chem. Educ. 1995, 72, 411.
Chemometrics
|
Spreadsheet-Controlled Potentiometric Analyses Mullin, Jerome; Marquardt, Michael
173. Bits and pieces, 53. Discussion of collecting experimental data on spreadsheets directly from laboratory instruments.
Mullin, Jerome; Marquardt, Michael J. Chem. Educ. 1995, 72, 400.
Laboratory Computing / Interfacing |
Chemometrics |
Potentiometry
|
Kinetics in Thermodynamic Clothing: Fun with Cooling Curves: A First-Year Undergraduate Chemistry Experiment Casadonte, Dominick J., Jr.
A series of experiments examining the phenomenon of cooling by producing part of the cooling curve for water at different initial temperatures, focussing on the fact that the curve is nonlinear (unlike the information presented in many texts).
Casadonte, Dominick J., Jr. J. Chem. Educ. 1995, 72, 346.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Kinetics
|
REACT: Exploring Practical Thermodynamic and Equilibrium Calculations Ramette, Richard W.
Description of REACT software to balance complicated equations; determine thermodynamic data for all reactants and products; calculate changes in free energy, enthalpy, and entropy for a reaction; and find equilibrium conditions for the a reaction.
Ramette, Richard W. J. Chem. Educ. 1995, 72, 240.
Stoichiometry |
Equilibrium |
Thermodynamics |
Chemometrics
|
Measuring with a Purpose: Involving Students in the Learning Process Metz, Patricia A.; Pribyl, Jeffrey R.
Constructivist learning activities for helping students to understand measurement, significant figures, uncertainty, scientific notation, and unit conversions.
Metz, Patricia A.; Pribyl, Jeffrey R. J. Chem. Educ. 1995, 72, 130.
Nomenclature / Units / Symbols |
Chemometrics |
Constructivism
|
Solution-Phase Thermodynamics: A "Spontaneity" Activity Bindel, Thomas H.
Experimental procedure for verifying the concept of spontaneity using solution chemistry; includes data and analysis.
Bindel, Thomas H. J. Chem. Educ. 1995, 72, 34.
Aqueous Solution Chemistry |
Thermodynamics
|
Periodic Trends for the Entropy of Elements Thoms, Travis
Graphical representation and explanation for periodic trends in the entropy of elements.
Thoms, Travis J. Chem. Educ. 1995, 72, 16.
Periodicity / Periodic Table |
Thermodynamics |
Main-Group Elements |
Transition Elements
|
Introducing Spreadsheet Data Analysis in the First-Semester Laboratory Bushey, Michelle M.
Massing a collection of pennies in order to introduce statistical concepts about small and large data sets as well as introduce students to the use of spreadsheets.
Bushey, Michelle M. J. Chem. Educ. 1994, 71, A90.
Chemometrics
|
Spreadsheet Statistics Simpson, John M.
Using computer spreadsheets to do statistical analysis on data.
Simpson, John M. J. Chem. Educ. 1994, 71, A88.
Chemometrics
|
Probing Student Misconceptions in Thermodynamics with In-Class Writing Beall, Herbert
Examples of the use of in-class writing assignments in the teaching of thermodynamics in general chemistry are presented.
Beall, Herbert J. Chem. Educ. 1994, 71, 1056.
Thermodynamics
|
Cooking Efficiencies of Pots and Pans Selco, Jodye I.
This article offers "real life" problems for heat capacity.
Selco, Jodye I. J. Chem. Educ. 1994, 71, 1046.
Heat Capacity |
Applications of Chemistry
|
Symbolic Algebra and Stoichiometry DeToma, Robert P.
Applying symbolic algebra (instead of the factor-label method) to stoichiometry calculations.
DeToma, Robert P. J. Chem. Educ. 1994, 71, 568.
Chemometrics |
Nomenclature / Units / Symbols
|
Rubber Elasticity: A Simple Method for Measurement of Thermodynamic Properties Byrne, John P.
A modified triple-beam balance that uses an optical lever to detect small changes in the length of a stretched rubber band.
Byrne, John P. J. Chem. Educ. 1994, 71, 531.
Thermodynamics |
Laboratory Equipment / Apparatus |
Physical Properties
|
A Simple Laboratory Experiment Using Popcorn To Illustrate Measurement Errors Kimbrough, Doris R.; Meglen, Robert R.
This experiment focuses on the difference between accuracy and precision and demonstrates the necessity for multiple measurements of an experimental variable.
Kimbrough, Doris R.; Meglen, Robert R. J. Chem. Educ. 1994, 71, 519.
Chemometrics
|
An Oscillating Reaction as a Demonstration of Principles Applied in Chemistry and Chemical Engineering Weimer, Jeffrey J.
Platinum catalyzed decomposition of methanol.
Weimer, Jeffrey J. J. Chem. Educ. 1994, 71, 325.
Thermodynamics |
Catalysis |
Transport Properties |
Kinetics |
Reactions
|
A Joke Based on Significant Figures Ruekberg, Ben
Joke to introduce significant figures.
Ruekberg, Ben J. Chem. Educ. 1994, 71, 306.
Chemometrics
|
Cryophori, Hot Molecules, and Frozen Nitrogen Hunter, Paul W. W.; Knoespel, Sheldon L.
Freezing water and nitrogen at low atmospheric pressure.
Hunter, Paul W. W.; Knoespel, Sheldon L. J. Chem. Educ. 1994, 71, 67.
Thermodynamics |
Phases / Phase Transitions / Diagrams
|
Photon-initiated hydrogen-chlorine reaction: A student experiment at the microscale level Egolf, Leanne M.; Keiser, Joseph T.
This lab offers a way to integrate the principles of thermodynamics and kinetics as well as other valuable instrumental methods.
Egolf, Leanne M.; Keiser, Joseph T. J. Chem. Educ. 1993, 70, A208.
Covalent Bonding |
Ionic Bonding |
Electrochemistry |
Free Radicals |
Microscale Lab |
Thermodynamics |
Kinetics
|
Solving equilibria problems with a graphing calculator: A robust method, free of algebra and calculus Ruch, David K.; Chasteen, T. G.
The method of successive approximations is frequently introduced in freshman chemistry as a means for solving equilibrium equations. However, this often requires an understanding of calculus that is problematic for introductory chemistry students. An alternative method to solving such equations is to use graphic calculators to solve problems graphically.
Ruch, David K.; Chasteen, T. G. J. Chem. Educ. 1993, 70, A184.
Equilibrium |
Chemometrics
|
Shell thickness of the copper-clad cent Vanselow, Clarence H.; Forrester, Sherri R.
An exercise in determining the thickness of the copper layer of modern pennies presents the opportunities to combine good chemistry, instrumentation, simple curve fitting, and geometry to solve a simply stated problem.
Vanselow, Clarence H.; Forrester, Sherri R. J. Chem. Educ. 1993, 70, 1023.
Metals |
Quantitative Analysis |
Chemometrics
|
How thick/thin is your mirror? McCullough, Thomas; Bell, Lisa
When a student reported that his/her water film was 6 cm thick, these authors felt a review of significant figures and dimensional analysis may be in order.
McCullough, Thomas; Bell, Lisa J. Chem. Educ. 1993, 70, 851.
Chemometrics
|
Measurement scales: Changing Celsius to Kelvin is not just a unit conversion Nordstrom, Brian H.
The key to understanding the difference between Celsius and Kelvin lies in the different types of measurement scales. Students may have an easier time manipulating equations (such as gas laws) if they knew the difference between these scales.
Nordstrom, Brian H. J. Chem. Educ. 1993, 70, 827.
Chemometrics |
Kinetic-Molecular Theory |
Gases
|
Statistical analysis of errors: A practical approach for an undergraduate chemistry lab: Part 1. The concepts Guedens, W. J.; Yperman, J.; Mullens, J.; Van Poucke, L. C.; Pauwels, E. J.
A concise and practice-oriented introduction to the analysis and interpretation of measurement and errors.
Guedens, W. J.; Yperman, J.; Mullens, J.; Van Poucke, L. C.; Pauwels, E. J. J. Chem. Educ. 1993, 70, 776.
Chemometrics
|
Introducing probabilistic concepts in chemistry: The preparation of 10-24 M solution as a limiting case de Vicente, M. Sastre
A straightforward dilution experiment that can be used as the starting point for establishing a link between chemistry and concepts of probability theory.
de Vicente, M. Sastre J. Chem. Educ. 1993, 70, 674.
Solutions / Solvents |
Chemometrics
|
AnswerSheets Cornelius, Richard
Review of a spreadsheet-based program that has modules on significant figures, VSEPR structures, stoichiometry, and unit conversions.
Cornelius, Richard J. Chem. Educ. 1993, 70, 460.
VSEPR Theory |
Stoichiometry |
Chemometrics
|
A mole of M&M's Merlo, Carmela; Turner, Kathleen E.
Engaging students by asking the question: How thick would the layer of M&M candies be if we covered the continental United States with a mole of these candies? Compare this to a mole of water.
Merlo, Carmela; Turner, Kathleen E. J. Chem. Educ. 1993, 70, 453.
Stoichiometry |
Chemometrics
|
AnswerSheets Cornelius, Richard
Review of a spreadsheet-like program that includes modules on significant figures, conversions, stoichiometry, and VSEPR structures.
Cornelius, Richard J. Chem. Educ. 1993, 70, 387.
VSEPR Theory |
Stoichiometry |
Chemometrics
|
Suggestions for truly evaluating texts Gordon, Glen E.
Suggestions for improvement in evaluating and publishing the analysis of textbooks in this Journal.
Gordon, Glen E. J. Chem. Educ. 1993, 70, 346.
Thermodynamics
|
Empirical formulas from atom ratios: A simple method to obtain the integer factors of a rational number Weltin, E.
Most textbooks advise students to use a method tantamount to trial and error when they encounter a ratio in empirical formula calculations where it is not immediately apparent what the coefficients should be. The author describes a simple procedure that is an effective way to find the integer factors.
Weltin, E. J. Chem. Educ. 1993, 70, 280.
Stoichiometry |
Chemometrics
|
Measuring Avogadro's number on the overhead projector Solomon, Sally; Hur, Chinhyu
A Petri dish filled with water and stearic acid dissolved in petroleum ether upon an overhead projector can be used to introduce the topic of Avogadro's number.
Solomon, Sally; Hur, Chinhyu J. Chem. Educ. 1993, 70, 252.
Chemometrics |
Stoichiometry
|
Using monetary analogies to teach average atomic mass Last, Arthur M.; Webb, Michael J.
Some strategies to overcome the frequent problem novice students have with calculating average atomic mass.
Last, Arthur M.; Webb, Michael J. J. Chem. Educ. 1993, 70, 234.
Chemometrics |
Stoichiometry
|
Relative atomic mass and the mole: A concrete analogy to help students understand these abstract concepts de Sanabia, Josefina Arce
Suggestions on how to improve student understandings of the mathematical idea of "ratio" to enhance conceptual understanding of this fundamental chemistry concept.
de Sanabia, Josefina Arce J. Chem. Educ. 1993, 70, 233.
Chemometrics |
Stoichiometry
|
Concept learning versus problem solving: There is a difference Nakhleh, Mary B.; Mitchell, Richard C.
Previous studies indicate that there is little connection between algorithmic problem solving skills and conceptual understanding. The authors provide some ways to evaluate students along a continuum of low-high algorithmic and conceptual problem solving skills. The study shows that current lecture method teaches students to solve algorithms rather than teaching chemistry concepts.
Nakhleh, Mary B.; Mitchell, Richard C. J. Chem. Educ. 1993, 70, 190.
Chemometrics |
Learning Theories |
Student-Centered Learning
|
An Investigative Density Experiment Samsa, Richard A.
A laboratory exercise about density that is engaging and allows students to use higher-level thinking skills and develop a plan to solve a problem.
Samsa, Richard A. J. Chem. Educ. 1993, 70, 149.
Laboratory Computing / Interfacing |
Chemometrics |
Physical Properties
|
More on the Question of Significant Figures Clase, Howard J.
Because so many students have a hard time understanding what significant figures are all about, this author developed a method using "?" to substitute for insignificant zeros. This helps many students finally grasp this convention.
Clase, Howard J. J. Chem. Educ. 1993, 70, 133.
Chemometrics
|
Equilibrium Calculator Allendoerfer, Robert
The equilibrium calculator can calculate the equilibrium concentrations of all reagents in an arbitrary chemical reaction with as many as five reactants and products.
Allendoerfer, Robert J. Chem. Educ. 1993, 70, 126.
Equilibrium |
Chemometrics
|
Heat and Work are Not "Forms of Energy" Peckham, Gavin D.; McNaught, Ian J.
Heat and work are processes by which the internal energy of a system is changed. The title reflects a common misconception used by students and instructors.
Peckham, Gavin D.; McNaught, Ian J. J. Chem. Educ. 1993, 70, 103.
Thermodynamics |
Enrichment / Review Materials
|
Ideas of Equality and Ratio: Mathematical Basics for Chemistry and the Fallacy of Unitary Conversion Ochiai, El-Ichiro.
The author argues against dimensional analysis (referred to as the "unitary conversion method" in this article) and champions the more elegant "ratio" or "equality" paradigms as a way to help students make sense of chemical equations and "de-algorithmize" chemical calculations at the introductory level.
Ochiai, El-Ichiro. J. Chem. Educ. 1993, 70, 44.
Chemometrics
|
Is Dimensional Analysis the Best We Have to Offer? Canagaratna, Sebastian G.
Dimensional analysis is a unit based approach while the alternative, "method of equations" is a relations-based approach to solving mathematical problems. The author argues that quantitative chemistry involves relationships between quantities and not units, making the later method more pedagogically sound.
Canagaratna, Sebastian G. J. Chem. Educ. 1993, 70, 40.
Chemometrics
|
Applying a simple linear least-squares algorithm to data with uncertainties in both variables Ogren, Paul J.; Norton, J. Russell
There are cases in which it is desirable to find an optimum linear least-squares fit to data with significant uncertainties in both the x and y variables.
Ogren, Paul J.; Norton, J. Russell J. Chem. Educ. 1992, 69, A130.
Chemometrics
|
Intensive and extensive: Underused concepts Canagaratna, Sebastian G.
Methods for teaching intensive and extensive properties.
Canagaratna, Sebastian G. J. Chem. Educ. 1992, 69, 957.
Physical Properties |
Thermodynamics
|
Determining the thermal expansion coefficient of gases Lehmann, Jochen K.
The authors improved the design of the apparatus and extended the experimental task on a recently published experiment for determining the zero point of the absolute temperature scale.
Lehmann, Jochen K. J. Chem. Educ. 1992, 69, 943.
Thermodynamics |
Gases |
Laboratory Equipment / Apparatus
|
An hydrogen sulfide free analytical technique for cation analysis: The statistical approach Gaggero, Fernando Labandera; Luaces, Victor Martinez
In this analysis the study of each cation was carried out independently without taking into account the other cations present in the solutions.
Gaggero, Fernando Labandera; Luaces, Victor Martinez J. Chem. Educ. 1992, 69, 934.
Chemometrics |
Qualitative Analysis |
Precipitation / Solubility
|
Classroom experience: Using estimated answers in solving chemistry problems Green, Michael E.; Garland, Denise A.
A textbook is described in which students solve all problems by estimation.
Green, Michael E.; Garland, Denise A. J. Chem. Educ. 1992, 69, 898.
Chemometrics |
Learning Theories
|
On the chemically impossible "other" roots in equilibrium calculations, II Ludwig, Oliver G.
In a previous paper the author described, using mathematics accessible to students, how an equilibrium calculation leading to a quadratic equation may be shown to have but one "chemical" root. The present work extends this demonstration to some reactions leading to cubic equations.
Ludwig, Oliver G. J. Chem. Educ. 1992, 69, 884.
Chemometrics |
Equilibrium
|
The metric system Mason, Lynn M.
Metric conversions commonly encountered in chemistry and biology, with tests over each lesson.
Mason, Lynn M. J. Chem. Educ. 1992, 69, 818.
Nomenclature / Units / Symbols |
Enrichment / Review Materials |
Chemometrics
|
A demonstration of the molar volume of nitrogen gas Hughes, Elvin, Jr.
A graphic illustration and a calculation of the approximate molar volume of nitrogen gas.
Hughes, Elvin, Jr. J. Chem. Educ. 1992, 69, 763.
Gases |
Chemometrics
|
Storing solar energy in calcium chloride Wilkins, Curtis C.; Hunter, Norman W.; Pearson, Earl F.
Using common chemistry concepts to determine the feasibility of storing solar energy in calcium chloride hexahydrate.
Wilkins, Curtis C.; Hunter, Norman W.; Pearson, Earl F. J. Chem. Educ. 1992, 69, 753.
Calorimetry / Thermochemistry |
Stoichiometry |
Chemometrics
|
A graphing activity to freshen up the laboratory Pribyl, Jeffrey R.
A laboratory activity designed to address students' difficulties in interpreting data from graphs and tables.
Pribyl, Jeffrey R. J. Chem. Educ. 1992, 69, 752.
Chemometrics
|
Putting some snap into work. Mitschele, Jonathan.
Suggestions for improving the instructional value of the demonstration presented.
Mitschele, Jonathan. J. Chem. Educ. 1992, 69, 687.
Thermodynamics
|
The thermodynamics of home-made ice cream. Gibbon, Donald L.; Kennedy, Keith; Reading, Nathan; Quieroz, Mardsen.
Using the production of ice cream to teach heat capacity, viscosity, and freezing-point reduction.
Gibbon, Donald L.; Kennedy, Keith; Reading, Nathan; Quieroz, Mardsen. J. Chem. Educ. 1992, 69, 658.
Thermodynamics |
Water / Water Chemistry |
Applications of Chemistry
|
First-year chemistry laboratory calculations on a spreadsheet Edwards, Paul A.; McKay, J. Brian; Sink, Charles W.
140. A laboratory exercise to introduce students to the use of computers and spreadsheets.
Edwards, Paul A.; McKay, J. Brian; Sink, Charles W. J. Chem. Educ. 1992, 69, 648.
Chemometrics
|
Applications of Maxwell-Boltzmann distribution diagrams. Peckham, Gavin D.; McNaught, Ian J.
Although Maxwell-Boltzmann distribution diagrams are intuitively appealing, care must be taken to avoid several common errors and misconceptions.
Peckham, Gavin D.; McNaught, Ian J. J. Chem. Educ. 1992, 69, 554.
Thermodynamics |
Rate Law |
Catalysis
|
A mole of salt crystals-Or how big is the Avogadro number? Hoyt, William.
Calculations designed to help students put the size of Avogadro's number into perspective.
Hoyt, William. J. Chem. Educ. 1992, 69, 496.
Nomenclature / Units / Symbols |
Chemometrics
|
Boiling and freezing simultaneously - with a feeble vacuum pump! Ellison, Mike
The author uses this demonstration of freezing and boiling at reduced pressure to reinforce concepts about energy effects in phase changes.
Ellison, Mike J. Chem. Educ. 1992, 69, 325.
Phases / Phase Transitions / Diagrams |
Water / Water Chemistry |
Thermodynamics
|
A simple but effective demonstration for illustrating significant figure rules when making measurements and doing calculations Zipp, Arden P.
Students can be surprised and confused when different arithmetical operations are performed on experimental data, because the rules change when changing from addition to subtraction to multiplication or division. The following is a simple way to illustrate several aspects of these rules.
Zipp, Arden P. J. Chem. Educ. 1992, 69, 291.
Chemometrics
|
Microstate York, Richard
Microstate allows experimentation with a simulated crystal that is viewed as a set of loosely coupled harmonic oscillators.
York, Richard J. Chem. Educ. 1992, 69, 130.
Crystals / Crystallography |
Thermodynamics
|
The conversion of chemical energy: Part 1. Technological examples Wink, Donald J.
When a chemical reaction occurs, the energy of the chemical species may change and energy can be released or absorbed from the surroundings. This can involve the exchange of chemical energy with another kind of energy or with another chemical system.
Wink, Donald J. J. Chem. Educ. 1992, 69, 108.
Reactions |
Thermodynamics |
Electrochemistry |
Photosynthesis
|
Studying odd-even effects and solubility behavior using alpha, omega-dicarboxylic acids Burrows, Hugh D.
Odd-even effect provides a satisfying way of introducing students to a large area of chemistry that encompasses both classical thermodynamics and applied aspects.
Burrows, Hugh D. J. Chem. Educ. 1992, 69, 69.
Precipitation / Solubility |
Physical Properties |
Thermodynamics
|
Spreadsheet titration of diprotic acids and bases Breneman, G. L.; Parker, O. J.
133. Bits and pieces, 47. A spreadsheet and chart, set up using Excel, for showing titration curves of any diprotic acid or base is described.
Breneman, G. L.; Parker, O. J. J. Chem. Educ. 1992, 69, 46.
Acids / Bases |
Chemometrics |
Titration / Volumetric Analysis
|
Small-scale thermochemistry experiment Brouwer, Henry
An inexpensive calorimeter that uses approximately 1/10 of the reagents required for the foam coffee cup.
Brouwer, Henry J. Chem. Educ. 1991, 68, A178.
Heat Capacity |
Thermodynamics |
Microscale Lab
|
Having fun with the metric system Campbell, Mark L.
A puzzle adds some fun to the mundane treatment of the metric system.
Campbell, Mark L. J. Chem. Educ. 1991, 68, 1043.
Chemometrics
|
Some conundrums of chemical nomenclature Quigley, Michael N.
When talking about chemistry, we use some awfully confusing terms that warrant scrutiny.
Quigley, Michael N. J. Chem. Educ. 1991, 68, 1009.
Chemometrics
|
The development of statistical concepts in a design-oriented laboratory course in scientific measuring Goedhart, Martin J.; Verdonk, Adri H.
This article offers a contribution to the development of curriculum that includes design and evaluation of measurements.
Goedhart, Martin J.; Verdonk, Adri H. J. Chem. Educ. 1991, 68, 1005.
Chemometrics
|
Chemical equations are actually matrix equations Alberty, Robert A.
Chemists tend to think that chemical equations are unique to chemistry and they are not used to thinking of chemical equations as the mathematical equations they in fact are. The objective of this paper is to illustrate the mathematical significance of chemical equations.
Alberty, Robert A. J. Chem. Educ. 1991, 68, 984.
Stoichiometry |
Chemometrics
|
KC? Discoverer: Exploring the properties of the chemical elements Liebel, Michael
This software program allows users to explore a large number of properties of the elements. The program can find all elements associated with a certain property, graph numeric properties against other numeric properties, list elements, sort elements, and use the periodic table to select elements.
Liebel, Michael J. Chem. Educ. 1991, 68, 956.
Periodicity / Periodic Table |
Physical Properties |
Chemometrics |
Descriptive Chemistry
|
A carbonate project introducing students to the chemistry lab Dudek, Emily
A description of a first semester general chemistry laboratory that helps acquaint students with a large variety of chemistry laboratory procedures.
Dudek, Emily J. Chem. Educ. 1991, 68, 948.
Chemometrics |
Gravimetric Analysis |
Titration / Volumetric Analysis |
Separation Science
|
The use of "marathon" problems as effective vehicles for the presentation of general chemistry lectures Burness, James H.
A marathon problem is a long, comprehensive, and difficult problem that ties together many of the topics in a chapter and that is solved together by the instructor and students. Sample problems are included and advantages and disadvantages of this approach are discussed.
Burness, James H. J. Chem. Educ. 1991, 68, 919.
Chemometrics
|
An SI mnemonic Quigley, M. N.
A mnemonic to help remember the physical quantities associated with the nine base SI units.
Quigley, M. N. J. Chem. Educ. 1991, 68, 815.
Chemometrics
|
The reusable heat pack McAfee, Lyle V.; Jumper, Charles F.
A commercial product that can be used to demonstrate thermodynamic principles.
McAfee, Lyle V.; Jumper, Charles F. J. Chem. Educ. 1991, 68, 780.
Thermodynamics
|
Developmental instruction: Part II. Application of the Perry model to general chemistry Finster, David C.
The Perry scheme offers a framework in which teachers can understand how students make meaning of their world, and specific examples on how instructors need to teach these students so that the students can advance as learners.
Finster, David C. J. Chem. Educ. 1991, 68, 752.
Learning Theories |
Atomic Properties / Structure |
Chemometrics |
Descriptive Chemistry
|
Grafit Lisensky, George C.
A data manipulation tool and plotting program useful at all levels of chemistry.
Lisensky, George C. J. Chem. Educ. 1991, 68, 587.
Laboratory Computing / Interfacing |
Chemometrics
|
Space-filling P-V-T models Hilton, Don B.
Space-filling models help beginning students visualize the numerical aspects of the empirical gas laws.
Hilton, Don B. J. Chem. Educ. 1991, 68, 496.
Gases |
Noncovalent Interactions |
Kinetic-Molecular Theory |
Chemometrics
|
When figures signify nothing Ahmad, Jamil
Significant figures in the "real world" set poor standards and confusing examples for chemistry students.
Ahmad, Jamil J. Chem. Educ. 1991, 68, 469.
Chemometrics
|
A call for simplification Schomaker, Verner; Waser, Jurg
Does "An Instructive Gibbs-Function Problem" unnecessarily confuse even the most capable students? An exchange of letters.
Schomaker, Verner; Waser, Jurg J. Chem. Educ. 1991, 68, 443.
Thermodynamics
|
A call for simplification Peterson, Donald
Does "An Instructive Gibbs-Function Problem" unnecessarily confuse even the most capable students? An exchange of letters.
Peterson, Donald J. Chem. Educ. 1991, 68, 443.
Thermodynamics |
Reactions
|
Solving quadratic equations to the correct number of significant figures Thomas, Rudolf
Presenting an application of the successive approximations method for solving quadratic or higher order expressions.
Thomas, Rudolf J. Chem. Educ. 1991, 68, 409.
Equilibrium |
Chemometrics
|
Is 8C equal to 50F? Thompson, H. Bradford
A play, commentary, modest proposal, and a "less modest" proposal regarding calculations and significant figures.
Thompson, H. Bradford J. Chem. Educ. 1991, 68, 400.
Chemometrics
|
The effect of context on the translation of sentences into algebraic equations Niaz, Mansoor; Herron, J. Dudley; Phelps, Amy J.
Assessing students in a one-semester preparatory chemistry course to see how well students understand proportional relationships.
Niaz, Mansoor; Herron, J. Dudley; Phelps, Amy J. J. Chem. Educ. 1991, 68, 306.
Chemometrics
|
The temperature and pressure dependence of the equilibrium properties of a system: Introducing thermodynamics in the classroom Solomon, Theodros
Introducing thermodynamics in the classroom in a manner that allows students to gain hints at the methods or approaches to be adopted.
Solomon, Theodros J. Chem. Educ. 1991, 68, 294.
Thermodynamics
|
Chemical equilibrium: III. A few math tricks Gordus, Adon A.
The third article in a series on chemical equilibrium that considers a few math "tricks" useful in equilibrium calculations and approximations.
Gordus, Adon A. J. Chem. Educ. 1991, 68, 291.
Acids / Bases |
Equilibrium |
Chemometrics |
Titration / Volumetric Analysis
|
Chemical equilibrium: II. Deriving an exact equilibrium equation Gordus, Adon A.
In this article appearing in a series on chemical equilibrium, authors consider how to derive a completely general equation for any chemical mixture.
Gordus, Adon A. J. Chem. Educ. 1991, 68, 215.
Equilibrium |
Chemometrics
|
A simple first-order consecutive rate reaction: A different method for its solution Hughes, Elvin, Jr.
Power series methods should be used whenever possible in chemistry courses.
Hughes, Elvin, Jr. J. Chem. Educ. 1991, 68, 180.
Chemometrics |
Equilibrium
|
A simple first-order consecutive rate reaction: A different method for its solution Castillo S., Carlos; Micolta S., Germania
A different way to present an equilibrium equation that appeared previously in this Journal.
Castillo S., Carlos; Micolta S., Germania J. Chem. Educ. 1991, 68, 179.
Chemometrics |
Equilibrium
|
Chemical equilibrium: I. The thermodynamic equilibrium constant Gordus, Adon A.
This is the first article in a series of eight that investigates the various assumptions that result in the simplified equilibrium equations found in most introductory texts. In this first article, the author considers the general nature of the constant K, Le Chatelier's principle, and the effect of the temperature on K.
Gordus, Adon A. J. Chem. Educ. 1991, 68, 138.
Thermodynamics |
Equilibrium
|
Finding largest common factors and simplest integer ratios Macomber, Roger S.
General chemistry students can ease some of their math-phobia with an exam question that deals with a familiar topic prior to putting these same mathematical principles into the context of chemistry.
Macomber, Roger S. J. Chem. Educ. 1991, 68, 42.
Chemometrics
|
Thermodynamic irreversibility Hollinger, Henry B.; Zenzen, Michael J.
Concepts of "reversible" and "irreversible" start out seeming simple enough, but students often become confused. This article tackles areas of confusion in hopes of providing clarity.
Hollinger, Henry B.; Zenzen, Michael J. J. Chem. Educ. 1991, 68, 31.
Kinetics |
Thermodynamics
|
SEQS 3.0 Student Version Simultaneous Equation Solver (Tucker, Edwin E.) Dierenfeldt, K.E.
SEQS 3.0 is a program of considerable versatility for solving sets of nonlinear simultaneous equations.
Dierenfeldt, K.E. J. Chem. Educ. 1990, 67, A149.
Chemometrics
|
A classroom experiment using the Pythagorean theorem in a discussion of the scientific method Sauls, Frederic, C.
Experiment to verify the Pythagorean theorem as a means of introducing the importance of accurate measurements, accuracy and error.
Sauls, Frederic, C. J. Chem. Educ. 1990, 67, 958.
Nonmajor Courses |
Chemometrics
|
Accuracy of measurements and the U.S. Census Gorin, George
Some aspects of taking the Census can help students to understand the problem of measurement error and the use of significant figures.
Gorin, George J. Chem. Educ. 1990, 67, 936.
Chemometrics
|
Lessons learned from Lord Rayleigh on the importance of data analysis Larsen, Russell D.
Analysis of the data collected by Lord Rayleigh in association with his discovery of argon presented as a model for scientific inquiry.
Larsen, Russell D. J. Chem. Educ. 1990, 67, 925.
Chemometrics |
Atmospheric Chemistry
|
ChemCalc: A scientific calculator Allendoerfer, Robert D.
A scientific calculator program that can be used as a stand-alone or incorporated into other software written in BASIC.
Allendoerfer, Robert D. J. Chem. Educ. 1990, 67, 770.
Chemometrics
|
A straightforward derivation of stoichiometric mass relationships Gorin, George
An alternative to the factor label method for solving stoichiometric mass relationship problems.
Gorin, George J. Chem. Educ. 1990, 67, 762.
Stoichiometry |
Chemometrics
|
A significant example: How many days in a century? Lisensky, George
Calculating the number of days in a century can help clarify the subject of significant figures.
Lisensky, George J. Chem. Educ. 1990, 67, 562.
Nomenclature / Units / Symbols |
Chemometrics
|
Experiments with "Calo-pH Meter" Paris, Michel R.; Aymes, Daniel J.
Paris, Michel R.; Aymes, Daniel J. J. Chem. Educ. 1990, 67, 510.
Laboratory Equipment / Apparatus |
Thermodynamics |
Calorimetry / Thermochemistry
|
Dynamic data storage in FORTRAN Chung-Phillips, Alice
115. Bits and pieces, 44. The purpose of this article is to promote the use of dynamic storage allocation in FORTRAN to chemistry instructors and students in the present computing environment.
Chung-Phillips, Alice J. Chem. Educ. 1990, 67, 500.
Chemometrics
|
Solving quadratic equations Brown, R. J. C.
A better technique than the quadratic equation for chemical equilibria is offered here.
Brown, R. J. C. J. Chem. Educ. 1990, 67, 409.
Chemometrics |
Equilibrium
|
An effective approach to teaching electrochemistry Birss, Viola I.; Truax, D. Rodney
By interweaving concepts from thermodynamics and chemical kinetics with those of electrochemical measurement, the authors provide students with an enriched appreciation of the utility of ideas from kinetics and thermodynamics.
Birss, Viola I.; Truax, D. Rodney J. Chem. Educ. 1990, 67, 403.
Electrochemistry |
Kinetics |
Thermodynamics
|
Introduction to experiment design for chemists Strange, Ronald S.
One purpose of this paper is to review basic concepts and terminology of experimental design, analysis of data, and optimization.
Strange, Ronald S. J. Chem. Educ. 1990, 67, 113.
Chemometrics
|
Calculating entropy changes at different extents of reaction Brosnan, Tim
The Revised Nuffield Chemistry course uses a simple statistical approach to entropy a a unifying idea in its treatment of thermodynamics. It was for these students that the author developed this method of calculating entropy changes at different extents of reaction which are listed here.
Brosnan, Tim J. Chem. Educ. 1990, 67, 48.
Thermodynamics
|
Exception to solving chem problems without the factor-label approach (the author replies) Cardulla, Frank
There are other ways to teach problem solving, and they can produce competent, successful, and enthusiastic students.
Cardulla, Frank J. Chem. Educ. 1989, 66, 1066.
Chemometrics |
Nomenclature / Units / Symbols
|
Exception to solving chem problems without the factor-label approach Gillette, Marcia L.
The classroom analogy Cardulla uses could be made much more meaningful if it were used to demonstrate the relation between what is obvious and what is not.
Gillette, Marcia L. J. Chem. Educ. 1989, 66, 1065.
Chemometrics |
Nomenclature / Units / Symbols
|
With Clausius from energy to entropy Baron, Maximo
Examination of entropy following the route taken by Clausius.
Baron, Maximo J. Chem. Educ. 1989, 66, 1001.
Thermodynamics
|
The acid-base package: A collection of useful programs for proton-transfer systems Hawkes, Stephen J.
Four programs that deal with the types of acid-base calculations normally encountered in introductory and analytical chemistry courses.
Hawkes, Stephen J. J. Chem. Educ. 1989, 66, 830.
Acids / Bases |
Chemometrics
|
Atlantic-Pacific sig figs Stone, Helen M.
Examples of applications of significant figures in calculations.
Stone, Helen M. J. Chem. Educ. 1989, 66, 829.
Nomenclature / Units / Symbols |
Chemometrics
|
How to visualize Avogadro's number van Lubeck, Henk
Three examples to help students visualize the size of a mole.
van Lubeck, Henk J. Chem. Educ. 1989, 66, 762.
Nomenclature / Units / Symbols |
Chemometrics
|
Significant figure rules for general arithmetic functions Graham, D. M.
Rules for determining what happens to the number of significant figures as various types of mathematical operations are performed upon certain quantities.
Graham, D. M. J. Chem. Educ. 1989, 66, 573.
Chemometrics
|
A stoichiometric journey Molle, Brian
A story to help students overcome some of the difficulties they encounter in stoichiometry calculations.
Molle, Brian J. Chem. Educ. 1989, 66, 561.
Stoichiometry |
Chemometrics
|
Being a participant in the future Parker, O. Jerry
Integrating computer technology into undergraduate chemistry courses.
Parker, O. Jerry J. Chem. Educ. 1989, 66, 500.
Administrative Issues |
Chemometrics
|
The relationship between M-demand, algorithms, and problem solving: A neo-Piagetian analysis Niaz, Mansoor
One of the most important implements developed by the neo-Piagetian theory is task analysis, that is, the evaluation of the M-demand of a problem. M-demand can be defined as: maximum number of steps that the subject must mobilize simultaneously in in the course of executing a task.
Niaz, Mansoor J. Chem. Educ. 1989, 66, 422.
Learning Theories |
Chemometrics
|
Significant Figures and Error Propagation West, Allen C.
Schwartz is wrong to say that 125 mL +/- 5% means a systematic error of +/-5%.
West, Allen C. J. Chem. Educ. 1989, 66, 272.
Chemometrics
|
Accurate equations of state in computational chemistry projects Allbee, David; Jones, Edward
101. This article presents one method that allows students to become familiar with the use of modern equations of state and also enhances their understanding of how computers can be used in the study and application of chemistry. [Includes "Editor's note: Changes in the computer series", by Lagowski, J. J., p. 226]
Allbee, David; Jones, Edward J. Chem. Educ. 1989, 66, 226.
Applications of Chemistry |
Chemometrics
|
Chemical generation and visualization of hydrodynamic instability: An extremely simple demonstration of self-organization Bowers, Peter G.; Soltzberg, Leonard J.
The chemical convection system described here is the pattern formation seen when an acidic vapor comes into contact with the surface of an aqueous solution containing indicator.
Bowers, Peter G.; Soltzberg, Leonard J. J. Chem. Educ. 1989, 66, 210.
Thermodynamics |
Aqueous Solution Chemistry |
Acids / Bases
|
A simple explanation of the salt water oscillator Noyes, Richard M.
Yoshikawa et al. have described a simple device that undergoes repeated oscillations and that can also illustrate some of the principles essential to the oscillators driven by chemical reactions.
Noyes, Richard M. J. Chem. Educ. 1989, 66, 207.
Laboratory Equipment / Apparatus |
Thermodynamics |
Equilibrium
|
Amusement with a salt-water oscillator Yoshikawa, Kenichi; Nakata, Satoshi; Yamanaka, Masahiro; Waki, Takeshi
Rhythmic oscillations of water flow are generated when a vertically oriented hypodermic syringe, with the plunger removed, is filled with salt water and partially submerged in a beaker of pure water.
Yoshikawa, Kenichi; Nakata, Satoshi; Yamanaka, Masahiro; Waki, Takeshi J. Chem. Educ. 1989, 66, 205.
Thermodynamics |
Equilibrium |
Laboratory Equipment / Apparatus
|
Some models of chemical oscillators Noyes, Richard M.
This review concentrates on models of chemical oscillations, which constitute the self-organization of a system in time without any accompanying organization in space.
Noyes, Richard M. J. Chem. Educ. 1989, 66, 190.
Thermodynamics
|
Self-organization in chemistry: The larger context Soltzberg, Leonard J.
The following three papers in this symposium will serve the reader as a good introduction to self-organization in chemical systems.
Soltzberg, Leonard J. J. Chem. Educ. 1989, 66, 187.
Thermodynamics
|
Visible spectrophotometric determination of the partition coefficient of methyl violet: A microscale extraction experiment Sonnenberger, David C.; Ferroni, Edward L.
This experiment is designed to demonstrate the principles of separation by solvent extraction, partition coefficient, and the construction and use of a Beer-Lambert standard curve.
Sonnenberger, David C.; Ferroni, Edward L. J. Chem. Educ. 1989, 66, 91.
Separation Science |
Chemometrics
|
Graphical analysis III (Vernier, David L.) Carpenter, Jeanette; Bowers, Caroline H.
Two reviews of a complete graphing tool suitable for high school and college applications with a wide range of operations varying in complexity.
Carpenter, Jeanette; Bowers, Caroline H. J. Chem. Educ. 1988, 65, A269.
Chemometrics
|
Chemistry according to ROF (Fee, Richard) Radcliffe, George; Mackenzie, Norma N.
Two reviews on a software package that consists of 68 programs on 17 disks plus an administrative disk geared toward acquainting students with fundamental chemistry content. For instance, acids and bases, significant figures, electron configuration, chemical structures, bonding, phases, and more.
Radcliffe, George; Mackenzie, Norma N. J. Chem. Educ. 1988, 65, A239.
Chemometrics |
Atomic Properties / Structure |
Equilibrium |
Periodicity / Periodic Table |
Periodicity / Periodic Table |
Stoichiometry |
Physical Properties |
Acids / Bases |
Covalent Bonding
|
Analysis of kinetic data with a spreadsheet program Henderson, John
An article about spreadsheet templates that accept concentration versus time data for several runs of an experiment, determination of least-squares lines through data points for each run, and will allow the user to exclude points from the least-squares calculation.
Henderson, John J. Chem. Educ. 1988, 65, A150.
Chemometrics |
Laboratory Computing / Interfacing |
UV-Vis Spectroscopy |
Rate Law |
Kinetics |
Enzymes
|
Two multipurpose thermochemical experiments for general chemistry Wentworth, R. A. D.
Two multipurpose thermochemical experiments are described in this paper.
Wentworth, R. A. D. J. Chem. Educ. 1988, 65, 1022.
Thermodynamics
|
Teaching students to use algorithms for solving generic and harder problems in general chemistry Kean, Elizabeth; Middlecamp, Catherine Hurt; Scott, D. L.
This paper describes teaching strategies that help students improve their problem-solving skills.
Kean, Elizabeth; Middlecamp, Catherine Hurt; Scott, D. L. J. Chem. Educ. 1988, 65, 987.
Stoichiometry |
Chemometrics
|
The Australian Academy of Science School Chemistry Project: A new-generation secondary school chemistry course Bucat, R. B.; Cole, A. R. H.
The purpose of this paper is to summarize the philosophies behind the courses described in this paper and the consequent design decisions regarding the selection and sequence of the chemistry content.
Bucat, R. B.; Cole, A. R. H. J. Chem. Educ. 1988, 65, 777.
Atmospheric Chemistry |
Metabolism |
Thermodynamics
|
Let's separate theories from calculations Freilich, Mark B.
This author writes in a 'provocative opinion' article challenging the readers to think about heavily emphasizing 'thought problems' in chemistry and allowing students to master those before throwing calculations into the mix.
Freilich, Mark B. J. Chem. Educ. 1988, 65, 442.
Chemometrics
|
An alternative to using the PV = nRT equation Desmarais, George
This author shares his application of the factor-label method to solving gas problems which involves using the ideal gas constant as the starting point in the relationship.
Desmarais, George J. Chem. Educ. 1988, 65, 392.
Gases |
Stoichiometry |
Chemometrics
|
Avogadro's number: A perverse view Lehman, Thomas A.
A way to think of Avogadro's number: take anything and double it 79 times.
Lehman, Thomas A. J. Chem. Educ. 1988, 65, 282.
Chemometrics |
Stoichiometry
|
The endothermic dissolution of ammonium nitrate Kauffman, George B.; Ferguson, Craig A.
A brief procedure for demonstrating the endothermic dissolution of ammonium nitrate.
Kauffman, George B.; Ferguson, Craig A. J. Chem. Educ. 1988, 65, 267.
Thermodynamics
|
Thermodynamics should be built on energy-not on heat and work Barrow, Gordon M.
This author looks closely at the concepts of heat, work, energy, and the laws of thermodynamics to back up his title argument.
Barrow, Gordon M. J. Chem. Educ. 1988, 65, 122.
Thermodynamics
|
Preparation of a simple thermochromic solid Van Oort, Michiel J. M.
An easy, dramatic, and effective laboratory introduction to solid-solid phase transitions, thermochromism, and color changes associated with changes in ligand coordination suitable for undergraduate students in physical and general chemistry.
Van Oort, Michiel J. M. J. Chem. Educ. 1988, 65, 84.
Phases / Phase Transitions / Diagrams |
Crystals / Crystallography |
Coordination Compounds |
Metals |
Thermodynamics
|
Remember E = hv is correct only half of the time Leo, Howard, R.
Reminder that the title equation (Planck) is not algebraically correct.
Leo, Howard, R. J. Chem. Educ. 1988, 65, 11.
Chemometrics |
Photochemistry
|
Correct equilibrium constants for water (the authors reply) Starkey, Ronald; Norman, Jack; Hinitze, Mark
Water and hydronium ion Ka values are special cases.
Starkey, Ronald; Norman, Jack; Hinitze, Mark J. Chem. Educ. 1987, 64, 1068.
Equilibrium |
Water / Water Chemistry |
Aqueous Solution Chemistry |
Acids / Bases |
Thermodynamics
|
Good numerical technique in chemistry: The quadratic equation Thompson, H. Bradford
Texts commonly avoid examples with bad round-off problems or handle them by approximation; none of this is necessary, for simple techniques are available to handle quadratic equations easily and precisely.
Thompson, H. Bradford J. Chem. Educ. 1987, 64, 1009.
Chemometrics
|
Reaction stoichiometry and suitable "coordinate systems" Tykodi, R. J.
Methods for dealing with problems involving reactions stoichiometry: unitize and scale up, factor-label procedure, de Donder ratios, and titration relations.
Tykodi, R. J. J. Chem. Educ. 1987, 64, 958.
Stoichiometry |
Titration / Volumetric Analysis |
Chemometrics
|
Converting sunlight to mechanical energy: A polymer example of entropy Mathias, Lon J.
Demonstrating entropy using an elastomer and a virtual foolproof "light engine".
Mathias, Lon J. J. Chem. Educ. 1987, 64, 889.
Thermodynamics
|
The entropy of dissolution of urea Pickering, Miles
This experiment combines colorimetric techniques, thermochemical techniques, some volumetric work, and actual measurements of entropy.
Pickering, Miles J. Chem. Educ. 1987, 64, 723.
Thermodynamics
|
Hard ways and easy ways Schwartz, Lowell M.
Two examples of common general chemistry calculations and different approaches ("hard" and "easy") to solving them.
Schwartz, Lowell M. J. Chem. Educ. 1987, 64, 698.
Stoichiometry |
Chemometrics
|
Enthalpy and Hot Wheels: An analogy Bonneau, Marcia C.
Demonstrating the relationship between activation energy and the heat of a reaction using a "Hot Wheels" track and car to simulate a potential energy diagram.
Bonneau, Marcia C. J. Chem. Educ. 1987, 64, 486.
Kinetics |
Calorimetry / Thermochemistry |
Thermodynamics
|
Solving limiting reagent problems (the author replies) Kalantar, A. H.
Thanks for clarification and suggestion.
Kalantar, A. H. J. Chem. Educ. 1987, 64, 472.
Stoichiometry |
Chemometrics
|
Solving limiting reagent problems Skovlin, Dean O.
Uncertainty in the meaning of the term X.
Skovlin, Dean O. J. Chem. Educ. 1987, 64, 472.
Stoichiometry |
Chemometrics
|
Statistical evaluation of class data for two buret readings Gordus, Adon A.
Data that serve to illustrate both random and systematic errors in measurements characteristic of titrations.
Gordus, Adon A. J. Chem. Educ. 1987, 64, 376.
Chemometrics |
Titration / Volumetric Analysis
|
Thermodynamics of the rhodamine B lactone zwitterion equilibrium: An undergraduate laboratory experiment Hinckley, Daniel A.; Seybold, Paul G.
An experiment to derive thermodynamic values from a thermochromic equilibrium that uses a commercially available dye, attains equilibrium rapidly, and employs a simple, single-beam spectrophotometer.
Hinckley, Daniel A.; Seybold, Paul G. J. Chem. Educ. 1987, 64, 362.
Thermodynamics |
Dyes / Pigments |
Spectroscopy |
Equilibrium
|
Mole fraction revisited Mancott, A.
This problem requires the use of algebraic reasoning to derive and solve a fraction linear equation based on the concept of moles and conservation of moles.
Mancott, A. J. Chem. Educ. 1987, 64, 320.
Stoichiometry |
Chemometrics
|
Thermodynamics and the bounce Carraher, Charles E., Jr.
Explaining the bouncing of a rubber ball using the laws of thermodynamics.
Carraher, Charles E., Jr. J. Chem. Educ. 1987, 64, 43.
Thermodynamics
|
Stretched elastomers: A case of decreasing length upon heating Clough, S. B.
Demonstrating and explaining the decrease in length of a heated rubber band.
Clough, S. B. J. Chem. Educ. 1987, 64, 42.
Thermodynamics |
Molecular Properties / Structure
|
Slopes of straight lines when neither axis is error free Kalantar, A. H.
The iterative effective variance method is not reliable and its use is pedagogically unwise.
Kalantar, A. H. J. Chem. Educ. 1987, 64, 28.
Chemometrics
|
Fire walking, temperature, and heat DeLorenzo, Ronald
Student interest piques when chemistry concepts are applied to this popular "trick".
DeLorenzo, Ronald J. Chem. Educ. 1986, 63, 976.
Thermodynamics
|
A new road to reactions: Part III. Teaching the heat effect of reactions de Vos, Wobbe; Verdonk, Adri H.
This series of work summarizes the authors' work on the concept of chemical reactions as a teaching and learning problem.
de Vos, Wobbe; Verdonk, Adri H. J. Chem. Educ. 1986, 63, 972.
Thermodynamics |
Reactions |
Solutions / Solvents |
Acids / Bases
|
The length of a pestle: A class exercise in measurement and statistical analysis O'Reilly, James E.
Too many students get through chemistry without acquiring a basic understanding and appreciation of the concepts of measurement science. The purpose of this report is to outline an extremely simple class exercise as a concrete paradigm of the entire process of making chemical measurements and treating data.
O'Reilly, James E. J. Chem. Educ. 1986, 63, 894.
Chemometrics
|
Calculation of Madelung constants in the first year chemistry course Elert, Mark; Koubek, Edward
76. Bits and pieces, 31. A computer program aids in understanding the nature of the Madelung constants.
Elert, Mark; Koubek, Edward J. Chem. Educ. 1986, 63, 840.
Crystals / Crystallography |
Chemometrics
|
Teaching significant figures using a learning cycle Guymon, E. Park; James, Helen J.; Saeger, Spencer L.
Can we teach significant figures in a way that will be better retained by our students? These authors propose a solution.
Guymon, E. Park; James, Helen J.; Saeger, Spencer L. J. Chem. Educ. 1986, 63, 786.
Learning Theories |
Chemometrics
|
A useful balloon demonstration: Pressure difference behavior Fenster, Ariel E.; Harpp, David N.; Schwarcz, Joseph A.
The authors contribute an interesting variant on the 'crushed can' experiment. [typo: first author's middle initial should be E.]
Fenster, Ariel E.; Harpp, David N.; Schwarcz, Joseph A. J. Chem. Educ. 1986, 63, 629.
Gases |
Thermodynamics
|
A flowchart for dimensional analysis Graham, D. M.
A flowchart to help students organize their thoughts when solving conversion problems.
Graham, D. M. J. Chem. Educ. 1986, 63, 527.
Chemometrics |
Nomenclature / Units / Symbols |
Stoichiometry
|
Where did that number come from? DeLorenzo, Ronald
With more careful labeling and handling of numbers, instructors can reduce the confusion students sometimes feel when watching problems being solved by the instructor on the board.
DeLorenzo, Ronald J. Chem. Educ. 1986, 63, 514.
Chemometrics |
Nomenclature / Units / Symbols
|
Factor-label: Another view Maloy, Joseph T.
It is of interest to our students' academic development that we teach them the mathematical theory behind factor label approaches to problems solving.
Maloy, Joseph T. J. Chem. Educ. 1986, 63, 186.
Chemometrics
|
Unit basis a neglected problem-solving technique Beichl, George J.
A technique that will prevent students from using ineffective problem-solving techniques such as dimensional analysis.
Beichl, George J. J. Chem. Educ. 1986, 63, 146.
Chemometrics |
Stoichiometry
|
Thermodynamics and reactions in the dry way Tykodi, Ralph J.
In dealing with reactions in the dry way, we can actually "see" in detail the workings of the thermodynamic machinery responsible for moving the reaction in the spontaneous direction. This note presents ideas at the general chemistry level.
Tykodi, Ralph J. J. Chem. Educ. 1986, 63, 107.
Thermodynamics |
Oxidation / Reduction
|
On writing equations Campbell, J.A.
The author presents a very direct approach to writing complicated equations without using a matrix approach.
Campbell, J.A. J. Chem. Educ. 1986, 63, 63.
Stoichiometry |
Chemometrics
|
An interactive, screen-oriented, general linear regression program Joshi, Bhairav D.
65. Bits and pieces, 26. Description of GSLINE, a program runs linear regressions.
Joshi, Bhairav D. J. Chem. Educ. 1985, 62, 1027.
Chemometrics
|
Mathematics in the chemistry classroom. Part 2. Elementary entities play their part Dierks, Werner; Weninger, Johann; Herron, J. Dudley
One of the problems that learners have to overcome when doing stoichiometry calculations is to learn how statements about elementary entities given by formulas and equations are related to statements about portions of substances as measured in the macroscopic world.
Dierks, Werner; Weninger, Johann; Herron, J. Dudley J. Chem. Educ. 1985, 62, 1021.
Chemometrics |
Stoichiometry
|
Pandemonium pesticide: A simple demonstration illustrating some fundamental chemical concepts Kauffman, George B.; Chooljian, Steven H.; Ebner, Ronald D.
Demonstration that uses large, visible particles to simulate calculations of atomic / molecular mass, percentage composition, and molecular formula.
Kauffman, George B.; Chooljian, Steven H.; Ebner, Ronald D. J. Chem. Educ. 1985, 62, 870.
Atomic Properties / Structure |
Molecular Properties / Structure |
Stoichiometry |
Chemometrics
|
Mathematics in the chemistry classroom. Part 1. The special nature of quantity equations Dierks, Werner; Weninger, Johann; Herron, J. Dudley
Differences between operation on quantities and operation on numbers and how chemical quantities should be described mathematically.
Dierks, Werner; Weninger, Johann; Herron, J. Dudley J. Chem. Educ. 1985, 62, 839.
Chemometrics |
Stoichiometry |
Nomenclature / Units / Symbols
|
Determination of molecular dimensions using monolayers: Another approach McNaught, Ian J.; Peckham, Gavin D.
A preliminary activity to help students understand the concept and calculations of the determination of molecular dimensions using monolayers.
McNaught, Ian J.; Peckham, Gavin D. J. Chem. Educ. 1985, 62, 795.
Molecular Properties / Structure |
Chemometrics
|
Propagation of significant figures Schwartz, Lowell M.
The rules of thumb for propagating significant figures through arithmetic calculations frequently yield misleading results.
Schwartz, Lowell M. J. Chem. Educ. 1985, 62, 693.
Chemometrics
|
Conversion of standard thermodynamic data to the new standard state pressure Freeman, Robert D.
Analyzes the changes that will be required to convert standard thermodynamic data from units of atmospheres to the bar.
Freeman, Robert D. J. Chem. Educ. 1985, 62, 681.
Thermodynamics |
Nomenclature / Units / Symbols
|
Energy interconversions in photosynthesis Bering, Charles L.
Reviews the energetics of the light reactions of photosynthesis.
Bering, Charles L. J. Chem. Educ. 1985, 62, 659.
Photosynthesis |
Photochemistry |
Thermodynamics |
Bioenergetics
|
A different look at the solubility-product principle Hugus, Z Z., Jr.; Hentz, F. C., Jr.
The progressive addition of Cl- to Ag+ yields an ion-product equal to Ksp at two different points.
Hugus, Z Z., Jr.; Hentz, F. C., Jr. J. Chem. Educ. 1985, 62, 645.
Precipitation / Solubility |
Aqueous Solution Chemistry |
Solutions / Solvents |
Chemometrics
|
Working backwards is a forward step in the solution of problems by dimensional analysis Drake, Robert F.
Solving chemistry calculations by determining the units of the desired answer and then working backwards using dimensional analysis.
Drake, Robert F. J. Chem. Educ. 1985, 62, 414.
Chemometrics |
Nomenclature / Units / Symbols
|
"Chemistry" problems without chemical terminology Ciereszko, Leon S.
Three questions analogous to percentage composition and Charles' law calculations.
Ciereszko, Leon S. J. Chem. Educ. 1985, 62, 402.
Chemometrics
|
Derivation of the ideal gas law Levine, S.
Derivation of the ideal gas law from a thermodynamic influence.
Levine, S. J. Chem. Educ. 1985, 62, 399.
Gases |
Thermodynamics |
Chemometrics
|
Using a conversion matrix to simplify stoichiometric calculations from balanced equations Berger, Selman A.
Two examples of using a conversion matrix to simplify stoichiometric calculations from balanced equations.
Berger, Selman A. J. Chem. Educ. 1985, 62, 396.
Chemometrics |
Stoichiometry
|
Problem-solving skills in chemistry made easier Fast, Kenneth V.
Step-by-step format for performing common calculations in chemistry.
Fast, Kenneth V. J. Chem. Educ. 1985, 62, 396.
Stoichiometry |
Chemometrics
|
A convenient device to demonstrate statistically based sampling error in a particulate mixture Reid, R. S.
Apparatus to demonstrate statistically based sampling error using a mixture of colored beads.
Reid, R. S. J. Chem. Educ. 1985, 62, 252.
Chemometrics
|
Le Châtelier's principle, temperature effects, and entropy Campbell, J. Arthur
A useful extension of Le Chatelier's Principle to predict concentration, pressure, and temperature effects solely from the equation for the net reaction.
Campbell, J. Arthur J. Chem. Educ. 1985, 62, 231.
Equilibrium |
Thermodynamics
|
Constant properties of systems: A rationale for the inclusion of thermodynamics in a high school chemistry course Schultz, Ethel L.
Using the zinc / copper system to illustrate how the thermodynamic functions can be introduced gradually and naturally into a course of study.
Schultz, Ethel L. J. Chem. Educ. 1985, 62, 228.
Thermodynamics
|
Should thermodynamics be X-rated? Bent, Henry A.
The benefits and detractions of teaching thermodynamics in high school and introductory college courses.
Bent, Henry A. J. Chem. Educ. 1985, 62, 228.
Thermodynamics
|
A gas kinetic explanation of simple thermodynamic processes Waite, Boyd A.
Proposes a simplified, semi-quantitative description of heat, work, and internal energy from the viewpoint of gas kinetic theory; both heat and work should not be considered as forms of energy but rather as different mechanisms by which internal energy is transferred from system to surroundings.
Waite, Boyd A. J. Chem. Educ. 1985, 62, 224.
Gases |
Kinetic-Molecular Theory |
Thermodynamics
|
Why isn't my rain as acidic as yours? Zajicek, O. T.
Calculating of pH values of acid rain and comparisons to uncontaminated samples.
Zajicek, O. T. J. Chem. Educ. 1985, 62, 158.
Acids / Bases |
Atmospheric Chemistry |
pH |
Chemometrics
|
Limiting reagent problems made simple for students Kalantar, A. H.
Method for determining the limiting reagent among three or more reactants.
Kalantar, A. H. J. Chem. Educ. 1985, 62, 106.
Stoichiometry |
Chemometrics
|
Five Avogadro's number problems Todd, David
Five problems involving Avogadro's number.
Todd, David J. Chem. Educ. 1985, 62, 76.
Nomenclature / Units / Symbols |
Stoichiometry |
Chemometrics
|
A LAP on moles: Teaching an important concept Ihde, John
The objective of the Learning Activity Packet on moles include understanding the basic concept of the mole as a chemical unit, knowing the relationships between the mole and the atomic weights in the periodic table, and being able to solve basic conversion problems involving grams, moles, atoms, and molecules. [Debut]
Ihde, John J. Chem. Educ. 1985, 62, 58.
Stoichiometry |
Nomenclature / Units / Symbols |
Chemometrics |
Atomic Properties / Structure |
Molecular Properties / Structure |
Periodicity / Periodic Table
|
Graphical Analysis, Review II (Dice, David R.) Sievers, Dennis
A computerized program that generates graphs of empirical data.
Sievers, Dennis J. Chem. Educ. 1984, 61, A324.
Chemometrics
|
Graphical Analysis, Review I (Dice, David R.) Palmer, Glenn E.
A computerized program that generates graphs of empirical data.
Palmer, Glenn E. J. Chem. Educ. 1984, 61, A323.
Chemometrics
|
The Elements of Style in Chemistry, A Computer-assisted Instruction Supported Text (Beatty, James W.; Beatty, James J.) Crawford, Victor A.
Intended to support students who have trouble solving important types of problems in chemistry.
Crawford, Victor A. J. Chem. Educ. 1984, 61, A27.
Enrichment / Review Materials |
Chemometrics
|
Thermo in the general chemistry course (the author replies) Schaffrath, Robert E.
A conceptual approach to thermodynamics is appropriate for general chemistry.
Schaffrath, Robert E. J. Chem. Educ. 1984, 61, 936.
Thermodynamics
|
Thermo in the general chemistry course Kimmell, Howard
A conceptual approach to thermodynamics is appropriate for general chemistry.
Kimmell, Howard J. Chem. Educ. 1984, 61, 936.
Thermodynamics
|
Further reflections on heat Hornack, Frederick M.
Confusion regarding the nature of heat and thermodynamics.
Hornack, Frederick M. J. Chem. Educ. 1984, 61, 869.
Kinetic-Molecular Theory |
Thermodynamics |
Calorimetry / Thermochemistry
|
Thermodynamic changes, kinetics, equilibrium, and LeChatelier's principle Hansen, Robert C.
A series of demonstrations in which water in beakers and the flow of water between beakers is used to represent the components of an exothermic chemical reaction and the flow and quantity of thermal energy involved in chemical changes.
Hansen, Robert C. J. Chem. Educ. 1984, 61, 804.
Equilibrium |
Kinetics |
Thermodynamics
|
Uncertainty analysis by the "worst case" method Gordon, Roy; Pickering, Miles; Bisson, Denise
A new method of uncertainty propagation that is in many ways superior to the traditional manipulation of absolute and relative uncertainty.
Gordon, Roy; Pickering, Miles; Bisson, Denise J. Chem. Educ. 1984, 61, 780.
Chemometrics
|
The factor-label method: Is it all that great? Navidi, Marjorie H.; Baker, A. David
The development of reasoning skills in chemistry is better achieved by postponing the introduction of the factor-label method.
Navidi, Marjorie H.; Baker, A. David J. Chem. Educ. 1984, 61, 522.
Chemometrics
|
The density of solids Burgess, Dale
Using density measurements as an opportunity to discuss experimental procedures, error, and significant figures.
Burgess, Dale J. Chem. Educ. 1984, 61, 242.
Chemometrics |
Physical Properties
|
Error in the minimum free energy curve Willis, Grover; Ball, David
Correction to the minimum free energy curve shown in some general chemistry texts.
Willis, Grover; Ball, David J. Chem. Educ. 1984, 61, 173.
Thermodynamics
|
A demonstration to aid in differentiating the concepts of heat and temperature Stevens, George H.
An easy, effective, "real world" demonstration on the distinction between heat and temperature. From "Using 'Real World' Examples in the Teaching of Chemistry - A Symposium", 7th BCCE, Stillwater OK, 1982.
Stevens, George H. J. Chem. Educ. 1983, 60, 1035.
Thermodynamics
|
Teaching factor-label method without sleight of hand Garrett, James M.
As an aid in teaching the factor-label method, the author has developed a rather simple card game involving the matching of symbols and colors.
Garrett, James M. J. Chem. Educ. 1983, 60, 962.
Stoichiometry |
Chemometrics |
Nomenclature / Units / Symbols
|
A bloody nose, the hairdresser's salon, flies in an elevator, and dancing couples: The use of analogies in teaching introductory chemistry Last, Arthur M.
The use of analogies can play an important role in assisting students in understanding some of the more difficult and/or abstract concepts in introductory chemistry. In addition, analogies can provide an amusing interlude during a lecture and can sometimes help a lecturer to interact with his students. The four analogies presented in this article represent some of the analogies students have found helpful and amusing in recent years.
Last, Arthur M. J. Chem. Educ. 1983, 60, 748.
Molecular Properties / Structure |
Kinetics |
Stoichiometry |
Thermodynamics
|
THERMPRO - A thermodynamics program Joshi, Bhairav D.
44. Bits and pieces, 16. THERMPRO is an interactive screen-oriented computer program written in BASICA for an IBM-PC with a graphics capability. It represents a general method of calculating standard thermodynamic properties of chemical reactions from heat capacity data for reactants and products.
Joshi, Bhairav D. J. Chem. Educ. 1983, 60, 733.
Thermodynamics
|
Reflections upon mathematics in the introductory chemistry course Goodstein, Madeline P.
It is the purpose of this paper to call attention to the lack of mathematical competence by chemistry students and to invite consideration of one conceptual scheme which may be used to unify the mathematical approach.
Goodstein, Madeline P. J. Chem. Educ. 1983, 60, 665.
Chemometrics |
Gases
|
On the chemically impossible "other" roots in equilibrium problems Ludwig, Oliver G.
Students often have a hard time knowing when to disregard equilibrium roots that are too large or are negative. The author suggests a convincing proof that helps students understand how the relationship between the conceptual and mathematical.
Ludwig, Oliver G. J. Chem. Educ. 1983, 60, 547.
Equilibrium |
Chemometrics
|
Empirical pKb and pKa for nonmetal hydrides from periodic table position Bayless, Philip L.
The equation in this article was developed by the author. It estimates the aqueous pKa for certain acids to an average deviation of 0.1pK unit for those with experimentally determined values and agrees with experimentally determined values, and as well as with estimates for those too weak or too strong to be measured.
Bayless, Philip L. J. Chem. Educ. 1983, 60, 546.
Acids / Bases |
pH |
Chemometrics
|
Le Châtelier's principle: the effect of temperature on the solubility of solids in liquids Brice, L. K.
The purpose of this article is to provide a rigorous but straightforward thermodynamic treatment of the temperature dependence of solubility of solids in liquids that is suitable for presentation at the undergraduate level. The present discussion may suggest how to approach the qualitative aspects of the subject for freshman.
Brice, L. K. J. Chem. Educ. 1983, 60, 387.
Thermodynamics |
Liquids |
Solids |
Chemometrics |
Equilibrium
|
Estimating energy outputs of fuels Baird, N. Colin
Which is the best fuel in terms of heat energy output: coal, natural gas, fuel oil, hydrogen, or alcohol? It is possible to obtain a semi quantitative estimate of the heat generated by combustion of a fuel from the balanced chemical equation alone.
Baird, N. Colin J. Chem. Educ. 1983, 60, 356.
Reactions |
Green Chemistry |
Thermodynamics |
Alcohols |
Alkanes / Cycloalkanes |
Geochemistry |
Stoichiometry |
Quantitative Analysis
|
The use of the Warnier-Orr program design method in the preparation of general chemistry tutorials Hach, Edwin E., Jr.
39. In this article, a modified Warnier-Orr approach is illustrated for a computer tutorial involving ideal gas calculations.
Hach, Edwin E., Jr. J. Chem. Educ. 1983, 60, 348.
Gases |
Chemometrics
|
The spilled can of paint Perkins, Robert
The writer describes a problem for students to work out in order to better understand units of conversion.
Perkins, Robert J. Chem. Educ. 1983, 60, 343.
Nomenclature / Units / Symbols |
Chemometrics
|
The liquid silver parade Perkins, Robert
The activity described in this note is useful in illustrating how small atoms are to students.
Perkins, Robert J. Chem. Educ. 1983, 60, 343.
Stoichiometry |
Chemometrics
|
Titration calculations- a problem-solving approach Waddling, Robin E. L.
This author shares a strategy for helping students who might be struggling with understanding how to calculate and understand titration data.
Waddling, Robin E. L. J. Chem. Educ. 1983, 60, 230.
Acids / Bases |
Titration / Volumetric Analysis |
Chemometrics
|
Solar energy experiment for beginning chemistry Davis, Clyde E.
This article introduces an experiment that incorporates chemical applications of solar energy into the curriculum.
Davis, Clyde E. J. Chem. Educ. 1983, 60, 158.
Thermodynamics |
Applications of Chemistry
|
Mass spectral analysis of halogen compounds Holdsworth, David K.
37. Bits and pieces, 14. A pocket calculator can be programmed to decide and display the halogen combination in a molecular-ion cluster by examination of the (M+2)/M or (X+2)/X percentage values.
Holdsworth, David K. J. Chem. Educ. 1983, 60, 103.
Chemometrics |
Mass Spectrometry
|
A pocket calculator program for the solution of pH problems via the method of successive approximations Guida, Wayne C.
37. Bits and pieces, 14. A description of a pocket calculator program for the solution of pH problems via the method of successive approximations .
Guida, Wayne C. J. Chem. Educ. 1983, 60, 101.
pH |
Acids / Bases |
Chemometrics
|
Data generation in the classroom Blanco, Luis H.
A pendulum device for generating data for statistical analysis.
Blanco, Luis H. J. Chem. Educ. 1982, 59, 1028.
Chemometrics |
Laboratory Equipment / Apparatus
|
The estimation of Avogadro's number using cetyl alcohol as the monolayer Feinstein, H. I.; Sisson, Robert F., III
Results and calculations using cetyl alcohol as the monolayer in estimating Avogadro's number.
Feinstein, H. I.; Sisson, Robert F., III J. Chem. Educ. 1982, 59, 751.
Stoichiometry |
Molecular Properties / Structure |
Chemometrics
|
Chemical equation balancing: A general method which is quick, simple, and has unexpected applications Blakley, G. R.
Using matrices to solve mathematical equations and balance chemical equations. From "The Goals of General Chemistry - A Symposium."
Blakley, G. R. J. Chem. Educ. 1982, 59, 728.
Stoichiometry |
Chemometrics
|
Chemical energy: A learning package Cohen, Ita; Ben-Zvi, Ruth
Problems associated with the teaching of chemical energy and an instructional package designed to overcome those difficulties.
Cohen, Ita; Ben-Zvi, Ruth J. Chem. Educ. 1982, 59, 656.
Thermodynamics |
Calorimetry / Thermochemistry
|
Entropy and its relation to work Richardson, W. S.
The relationship of entropy to the disorder of a system can be explained using a deck of playing cards.
Richardson, W. S. J. Chem. Educ. 1982, 59, 649.
Thermodynamics
|
Mathematics in data analysis: An introduction Wang, Taitzer
The meaning of simple mathematical equations are described in a perspective that, for some reasons, many beginning students do not seem to be able to obtain from reading textbooks on the subject.
Wang, Taitzer J. Chem. Educ. 1982, 59, 592.
Chemometrics
|
Recurrent difficulties: Solving quantitative problems Kramers-Pals, H.; Lambrechts, J.; Wolff, P. J.
Investigating the process students use to solve quantitative problems using a think aloud strategy.
Kramers-Pals, H.; Lambrechts, J.; Wolff, P. J. J. Chem. Educ. 1982, 59, 509.
Chemometrics
|
Entropy and its role in introductory chemistry Bickford, Franklin R.
The concept of entropy as it applies to phase changes.
Bickford, Franklin R. J. Chem. Educ. 1982, 59, 317.
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Solids |
Liquids |
Gases
|
Remedial mathematics for the introductory chemistry course: The "CHEM. 99" concept Bohning, James J.
An approach that is aimed specifically at mathematical deficiencies and based on the premise that the deductive reasoning process that accompanies basic mathematical technique is crucial for a meaningful comprehension of general chemistry principles.
Bohning, James J. J. Chem. Educ. 1982, 59, 207.
Chemometrics
|
Buffers Gold, Marvin
A demonstration based on buffer calculations.
Gold, Marvin J. Chem. Educ. 1982, 59, 155.
Acids / Bases |
Chemometrics
|
Calculation of statistical thermodynamic properties Vicharelli, P. A.; Collins, C. B.
25. Bits and pieces, 9. A computer program for the calculation of specific heat, entropy, enthalpy, and Gibbs free energy of polyatomic molecules.
Vicharelli, P. A.; Collins, C. B. J. Chem. Educ. 1982, 59, 131.
Calorimetry / Thermochemistry |
Thermodynamics |
Chemometrics
|
CAI Programs in BASIC and an associated MATH subroutine Anderson, Robert Hunt
25. Bits and pieces, 9. Four BASIC programs involving basic calculations and mathematical problems in chemistry.
Anderson, Robert Hunt J. Chem. Educ. 1982, 59, 129.
Chemometrics |
Enrichment / Review Materials
|
Basic mathematics for beginning chemistry (Goldish, Dorthoy M.) Ellison, Herbert R.
Ellison, Herbert R. J. Chem. Educ. 1981, 58, A65.
Chemometrics |
Mathematics / Symbolic Mathematics |
Enrichment / Review Materials
|
Think Wheeler, S. J., James D.
Students have an easy enough time crunching numbers, but it is alarming how little they understand the concepts behind the numbers. Students should not be making remarks such as, "If they keep changing how they write the problems, how am I supposed to know how to solve them?"
Wheeler, S. J., James D. J. Chem. Educ. 1981, 58, 1004.
Learning Theories |
Chemometrics
|
Weight-loss diets and the law of conservation of energy Hill, John W.
The law of conservation of mass is has real-life relevance to those who diet to lose weight.
Hill, John W. J. Chem. Educ. 1981, 58, 996.
Metabolism |
Thermodynamics
|
Small things and large numbers Rosenberg, Milton H.
Some challenging solubility problems are featured in this note.
Rosenberg, Milton H. J. Chem. Educ. 1981, 58, 962.
Solutions / Solvents |
Equilibrium |
Chemometrics
|
Superlative problems Akers, Hugh A.; Akers, Gwyn E.
The data in the Guinness Book of World Records holds great potential for fun, interesting chemistry exercises.
Akers, Hugh A.; Akers, Gwyn E. J. Chem. Educ. 1981, 58, 795.
Chemometrics
|
Entropy rules in my class too! White, Alvan D.
A simple analogy that will help students understand entropy.
White, Alvan D. J. Chem. Educ. 1981, 58, 645.
Thermodynamics
|
Be a millionaire - Get with the action! White, Alvan D.
When talking about the distribution of molecular velocities, we can use money as an analogy.
White, Alvan D. J. Chem. Educ. 1981, 58, 645.
Reactions |
Thermodynamics
|
Balancing complex redox equations by inspection Kolb, Doris
A step-by-step walk through of the inspection process for balancing equations.
Kolb, Doris J. Chem. Educ. 1981, 58, 642.
Stoichiometry |
Chemometrics
|
A statistical note on the time lag method for second-order kinetic rate constants Schwartz, Lowell M.
A clever method for finding second-order kinetic rate constants by using a time lag method that avoids direct measurement of the end point reading P(infinity) can easily be programmed.
Schwartz, Lowell M. J. Chem. Educ. 1981, 58, 588.
Chemometrics |
Kinetics |
Rate Law
|
A mathematics readiness test for prospective chemistry students Weisman, Rence L.
A mathematics readiness test is prepared to determine whether students have the minimum competency necessary to succeed in chemistry.
Weisman, Rence L. J. Chem. Educ. 1981, 58, 564.
Chemometrics |
Mathematics / Symbolic Mathematics
|
An illustration of applied calorimetry - Dieting students Perkins, Robert R.
The author shares a question that catches student interest and exemplifies the theoretical concepts of calorimetry.
Perkins, Robert R. J. Chem. Educ. 1981, 58, 548.
Calorimetry / Thermochemistry |
Thermodynamics |
Applications of Chemistry
|
How big is Avogadro's number (or how small are atoms, molecules and ions) Fulkrod, John E.
Calculating the volume occupied by Avogadro's number of drops of water helps students understand the magnitude of this quantity while giving them practice at using scientific notation and the metric system.
Fulkrod, John E. J. Chem. Educ. 1981, 58, 508.
Nomenclature / Units / Symbols |
Chemometrics |
Stoichiometry
|
Pressure and the exploding beverage container Perkins, Robert R.
The question in this article is an extension of exploding pop bottles to illustrate the balancing of a chemical equation, enthalpy, stoichiometry, and vapor pressure calculations, and the use of the Ideal Gas Equation. The question is aimed at the first-year level student.
Perkins, Robert R. J. Chem. Educ. 1981, 58, 363.
Stoichiometry |
Gases |
Thermodynamics |
Chemometrics
|
Entropy as a driving force Salzsieder, John C.
An inexpensive demonstration that requires virtually no setup time (and always works!) can be used to illustrate the driving force of entropy.
Salzsieder, John C. J. Chem. Educ. 1981, 58, 280.
Thermodynamics
|
Maxwell's demon Schmuckler, Joseph S.
Schmuckler, Joseph S. J. Chem. Educ. 1981, 58, 183.
Reactions |
Thermodynamics |
Precipitation / Solubility |
Calorimetry / Thermochemistry |
Kinetics |
Rate Law
|
Maxwell's demon Schmuckler, Joseph S.
Schmuckler, Joseph S. J. Chem. Educ. 1981, 58, 183.
Reactions |
Thermodynamics |
Precipitation / Solubility |
Calorimetry / Thermochemistry |
Kinetics |
Rate Law
|
A specific heat analogy McCullough, Brother Thomas, CSC
An analogy for helping students to understand the concepts of specific heat and heat transfer problems.
McCullough, Brother Thomas, CSC J. Chem. Educ. 1980, 57, 896.
Calorimetry / Thermochemistry |
Chemometrics
|
Sweet heat O'Connor, Rod
What would be the net enthalpy change for the complete combustion of 5.00 g of glucose at body temperature?
O'Connor, Rod J. Chem. Educ. 1980, 57, 889.
Carbohydrates |
Calorimetry / Thermochemistry |
Chemometrics
|
Teaching and learning problem solving in science. Part I: A general strategy Mettes, C. T. C. W.; Pilot, A.; Roossink, H. J.; Kramers-Pals, H.
A systematic approach to solving problems and on designing instruction where students learn this approach.
Mettes, C. T. C. W.; Pilot, A.; Roossink, H. J.; Kramers-Pals, H. J. Chem. Educ. 1980, 57, 882.
Chemometrics
|
Empirical formulas - A ratio problem Knox, Kerro
A problem involving an analogy between ratios of boys to girls given their average weights and percentage composition of the class by weight.
Knox, Kerro J. Chem. Educ. 1980, 57, 879.
Chemometrics |
Molecular Properties / Structure
|
Mole fraction analogies DeLorenzo, Ron
An analogy to help students solve concentration problems.
DeLorenzo, Ron J. Chem. Educ. 1980, 57, 733.
Stoichiometry |
Chemometrics |
Solutions / Solvents
|
Stormy weather Taylor, Thomas E.
Question regarding the formation of rain clouds and the exothermic process of condensation.
Taylor, Thomas E. J. Chem. Educ. 1980, 57, 732.
Thermodynamics |
Atmospheric Chemistry |
Water / Water Chemistry |
Phases / Phase Transitions / Diagrams
|
Dissociation of a weak acid Ladd, M. F. C.
An earlier treatment of the equilibrium of a weak acid in water gives, for certain ranges of concentration, significantly incorrect results.
Ladd, M. F. C. J. Chem. Educ. 1980, 57, 669.
Acids / Bases |
Aqueous Solution Chemistry |
Equilibrium |
Chemometrics
|
A "road map" problem for freshman chemistry students Burness, James H.
Question suitable for a take-home type of exam.
Burness, James H. J. Chem. Educ. 1980, 57, 647.
Gases |
Solutions / Solvents |
Stoichiometry |
Nomenclature / Units / Symbols |
Chemometrics
|
Significant figures: Removing the zero mystique Treptow, Richard S.
Zeros are significant if they appear before a number takes on size or as stand-ins for unknown digits.
Treptow, Richard S. J. Chem. Educ. 1980, 57, 646.
Chemometrics
|
Whatever became of significant figures? The trend toward numerical illiteracy Anderlik, Barbara
How does one persuade students, when working with physical measurements, to part with excess digits and become numerically literate.
Anderlik, Barbara J. Chem. Educ. 1980, 57, 591.
Chemometrics
|
An illustration to demonstrate the smallness of molecules Kingston, David W.
An exercise in dimensional analysis.
Kingston, David W. J. Chem. Educ. 1980, 57, 506.
Chemometrics
|
Correlating Celsius and Fahrenheit temperatures by the "unit calculus" Gorin, George
Deriving the mathematical relationship between Celsius and Fahrenheit temperatures.
Gorin, George J. Chem. Educ. 1980, 57, 350.
Nomenclature / Units / Symbols |
Chemometrics
|
Adopting SI units in introductory chemistry Davies, William G.; Moore, John W.
Conventions associated with SI units, conversion relationships commonly used in chemistry, and a roadmap method for solving stoichiometry problems.
Davies, William G.; Moore, John W. J. Chem. Educ. 1980, 57, 303.
Nomenclature / Units / Symbols |
Chemometrics
|
Adding another dimension to dimensional analysis DeLorenzo, Ronald
Adding words to typical dimensional analysis work to improve understanding and communication.
DeLorenzo, Ronald J. Chem. Educ. 1980, 57, 302.
Chemometrics
|
Paradigms and paradoxes Campbell, J. A.
Examines the commonly held tenets "systems tend to a minimum potential energy," "the entropy of a shuffled deck of cards is greater than that of a new deck," and "energy is the ability to do work."
Campbell, J. A. J. Chem. Educ. 1980, 57, 41.
Thermodynamics
|
Significant digits: Numbers and their logarithms Clever, H. Lawrence
The number of digits to report in a base 10 logarithm is an unresolved problem for many students.
Clever, H. Lawrence J. Chem. Educ. 1979, 56, 824.
Chemometrics |
pH
|
Corrosion: A Waste of energy J. Chem. Educ. Staff
Thermodynamics and electrochemical aspects of corrosion, and inhibition of the corrosion process.
J. Chem. Educ. Staff J. Chem. Educ. 1979, 56, 673.
Oxidation / Reduction |
Applications of Chemistry |
Metals |
Thermodynamics |
Electrochemistry
|
The physically meaningful solution of the quadratic equation Levy, Mel; Byers, Larry D.
Shows that the potential ambiguity of two unequal but physically meaningful roots never arises.
Levy, Mel; Byers, Larry D. J. Chem. Educ. 1979, 56, 526.
Chemometrics
|
Calculators in freshman chemistry - An alternative view Gold, Marvin
There is a serious negative aspect to allowing freshmen use of calculators in chemistry.
Gold, Marvin J. Chem. Educ. 1979, 56, 526.
Chemometrics
|
Why thermodynamics should not be taught to freshmen, or who owns the problem? Battino, Rubin
Thermodynamics should not be taught to freshmen - there are better things to do with the time.
Battino, Rubin J. Chem. Educ. 1979, 56, 520.
Thermodynamics
|
What thermodynamics should be taught to freshmen, or what is the goal? Campbell, J. A.
The great majority of students in first-year college courses must try to work problems involving changes in enthalpy, entropy, and Gibbs Free Energy.
Campbell, J. A. J. Chem. Educ. 1979, 56, 520.
Thermodynamics
|
Bond free energies Amador, Alberto
Provides standard free energies for the formation of common single and multiple bonds.
Amador, Alberto J. Chem. Educ. 1979, 56, 453.
Covalent Bonding |
Thermodynamics
|
Compact Compacts Huebner, Jay S.; Shiflett, R. B.; Blanck, Harvey F.
A collection of three suggestions regarding demonstrating the oxidation of hydrocarbons and the primary, secondary, and tertiary structure of proteins and the first law of thermodynamics as applied to air conditioning.
Huebner, Jay S.; Shiflett, R. B.; Blanck, Harvey F. J. Chem. Educ. 1979, 56, 389.
Oxidation / Reduction |
Alkanes / Cycloalkanes |
Molecular Properties / Structure |
Proteins / Peptides |
Thermodynamics
|
Comments on the criterion of spontaneity Senozan, N. M.
Draws attention to the incomplete or misleading presentations sometimes made in connection with the criteria for spontaneous reactions.
Senozan, N. M. J. Chem. Educ. 1979, 56, 381.
Thermodynamics
|
An apparent contradiction in the application of the principle of Le Chtelier Mellon, E. K.
Unless some care is exercised, the application of free energy concepts in situations where marked temperature changes occur can lead to apparent contradictions like the one described in this paper.
Mellon, E. K. J. Chem. Educ. 1979, 56, 380.
Equilibrium |
Thermodynamics
|
Entropy and rubbery elasticity Nash, Leonard K.
Thermodynamic analysis of the polymeric molecules of rubber.
Nash, Leonard K. J. Chem. Educ. 1979, 56, 363.
Thermodynamics |
Molecular Properties / Structure |
Statistical Mechanics
|
A freshman chemistry thermodynamics experiment: The cyclic rule revisited Dezube, Bruce
A verification of the cyclic rule through measurements of a stretched rubber band.
Dezube, Bruce J. Chem. Educ. 1979, 56, 313.
Thermodynamics
|
Measurement errors: A lecture demonstration Munn, Robert J.
A lecture demonstration to realistically discuss precision, accuracy, averaging, data rejection, and significant digits.
Munn, Robert J. J. Chem. Educ. 1979, 56, 267.
Chemometrics
|
How many significant digits in 0.05C? Power, James D.
Textbooks abound with erroneous examples, such as 33F = 0.56C.
Power, James D. J. Chem. Educ. 1979, 56, 239.
Chemometrics |
Nomenclature / Units / Symbols
|
Calculators, slide rules, and significant figures McCullough, Thomas, CSC
Using a slide rule to help students understand the concept of significant figures before using a calculator.
McCullough, Thomas, CSC J. Chem. Educ. 1979, 56, 238.
Chemometrics
|
Thermodynamics and solubilities of salts of dipositive ions Riley, Gary F.; Eberhardt, William H.
Used to illustrate the application of the principle that a decrease in free energy is a criterion for the spontaneity of a chemical reaction.
Riley, Gary F.; Eberhardt, William H. J. Chem. Educ. 1979, 56, 206.
Thermodynamics |
Precipitation / Solubility |
Physical Properties |
Reactions
|
Intuitive and general approach to acid-base equilibrium calculations Felty, Wayne L.
The purpose of this paper is to show that the usual intuitive approach used in general chemistry can be readily extended without introduction of additional, sophisticated concepts to give the general, exact expression and to point out the pedagogical advantage of its use.
Felty, Wayne L. J. Chem. Educ. 1978, 55, 576.
Acids / Bases |
Equilibrium |
Chemometrics
|
Pressure calculations Schultz, Charles W.
This question requires students to be able to distinguish two kinds of pressure: Boyles law pressure of gas (that depends on volume) from the equilibrium vapor pressure above a liquid (that does not).
Schultz, Charles W. J. Chem. Educ. 1978, 55, 515.
Gases |
Chemometrics
|
I. How much work can a person do? Bent, Henry A.
This article relates concepts of work and energy by walking through a calculation of how much work is produced during exercise. [Debut]
Bent, Henry A. J. Chem. Educ. 1978, 55, 456.
Thermodynamics |
Biophysical Chemistry
|
A Demonstration of burning magnesium and dry ice Driscoll, Jerry A.
This demonstration is a new, exciting approach to an older demonstration.
Driscoll, Jerry A. J. Chem. Educ. 1978, 55, 450.
Thermodynamics |
Kinetics |
Reactions
|
Hammond's postulate and the slinky Macomber, Roger S.
The transition state of a one-step chemical reaction is one of the most fundamental concepts in chemistry. The author shares an in-class analogy that can be used to help students understand this concept better.
Macomber, Roger S. J. Chem. Educ. 1978, 55, 449.
Thermodynamics
|
Balancing an atypical redox equation Carrano, S. A.
The author presents a particularly tricky redox problem and walks readers through a solution.
Carrano, S. A. J. Chem. Educ. 1978, 55, 382.
Chemometrics |
Oxidation / Reduction |
Stoichiometry
|
Chemical predictions from pKa values Hassanali, A.
The problem presented here develops student understanding of both pKa calculations and organic acids.
Hassanali, A. J. Chem. Educ. 1978, 55, 378.
Acids / Bases |
pH |
Chemometrics
|
Teaching the method of successive approximations Nassiff, Peter J.; Boyko, E. R.
The purpose of this papers is to help the teacher show the student why basic methods of successive approximations work, how they may be applied, and under what conditions it will be successful.
Nassiff, Peter J.; Boyko, E. R. J. Chem. Educ. 1978, 55, 376.
Chemometrics |
Acids / Bases |
Gases
|
Variation of radioactive decay rates Wolsey, Wayne C.
133. It is stated frequently in introductory chemistry texts that radioactive decay rates are invariant. Students are led to the impression, implicitly, if not explicitly, that changes in chemical form, temperature, pressure, etc. have no effect upon the half-lives of unstable nuclei. This constancy of decay is perhaps true for some particular modes of decay, but by no means is it true for all.
Wolsey, Wayne C. J. Chem. Educ. 1978, 55, 302.
Nuclear / Radiochemistry |
Thermodynamics
|
Collision theory Myers, Richard S.
The question presented here can be employed in general or physical chemistry courses.
Myers, Richard S. J. Chem. Educ. 1978, 55, 243.
Chemometrics |
Thermodynamics |
Kinetics
|
The chemical equation. Part I: Simple reactions Kolb, Doris
A chemical equation is often misunderstood by students as an "equation" that is used in chemistry. However, a more accurate description is that it is a concise statement describing a chemical reaction expressed in chemical symbolism.
Kolb, Doris J. Chem. Educ. 1978, 55, 184.
Stoichiometry |
Chemometrics |
Nomenclature / Units / Symbols |
Reactions
|
General chemistry thermodynamics experiment Beaulieu, Lynn P., CPT
An experiment is outlined here that provides students with an opportunity to do experimental thermodynamics, and to calculate those thermodynamic values which usually cannot be determined with the simple equipment available in a general chemistry laboratory.
Beaulieu, Lynn P., CPT J. Chem. Educ. 1978, 55, 53.
Thermodynamics
|
Teaching about "why do chemical reactions occur": Gibbs free energy Vamvakis, Steven N.; Schmuckler, Joseph S.
Approaching the topic of Gibbs free energy from the student's prior experience in algebra and geometry, it is possible to construct a proof that should enable students to explain the derivation of G = H - TS.
Vamvakis, Steven N.; Schmuckler, Joseph S. J. Chem. Educ. 1977, 54, 757.
Thermodynamics |
Reactions
|
Lecture table experimental demonstration of entropy Dole, Malcolm
Apparatus for demonstrating entropy that involves heating a stretched rubber band with hot steam.
Dole, Malcolm J. Chem. Educ. 1977, 54, 754.
Thermodynamics
|
A pre-general chemistry course for the underprepared student Krannich, Larry K.; Patick, David; Pevear, Jesse
Outline and evaluation of a course in chemical problem solving.
Krannich, Larry K.; Patick, David; Pevear, Jesse J. Chem. Educ. 1977, 54, 730.
Enrichment / Review Materials |
Chemometrics
|
Le Chtelier's principle demonstrated with a rubber band Smith, Douglas D.
Heating a rubber band causes it to contract and stretching it causes it to become warmer.
Smith, Douglas D. J. Chem. Educ. 1977, 54, 701.
Equilibrium |
Thermodynamics
|
Chemical equilibrium: Analogies that separate the mathematics from the chemistry DeLorenzo, Ronald A.
Demonstrates that the mathematics of chemical equilibria are not difficult, particularly when put in a non-chemical context.
DeLorenzo, Ronald A. J. Chem. Educ. 1977, 54, 676.
Equilibrium |
Chemometrics
|
On significant figures MacCarthy, Patrick
Illustrating the decrease in uncertainty that accompanies an increase in significant figures.
MacCarthy, Patrick J. Chem. Educ. 1977, 54, 578.
Chemometrics
|
Using oxidation state diagrams to teach thermodynamics and inorganic chemistry Friedel, A.; Murray, R.
Using oxidation state diagrams is suggested as a means of solving some of the problems associated with the teaching of thermodynamics and inorganic group chemistry.
Friedel, A.; Murray, R. J. Chem. Educ. 1977, 54, 485.
Thermodynamics |
Oxidation State
|
Simple classroom experiment on uncertainty of measurement Sen, B.
This activity demonstrates several aspects regarding the statistical treatment of data.
Sen, B. J. Chem. Educ. 1977, 54, 468.
Chemometrics
|
Free energy surfaces and transition state theory Cruickshank, F. R.; Hyde, A. J.; Pugh, D.
130/131. Unless free energy diagrams are very precisely labeled and explained they are seriously misleading and often incorporate a major error of principle. [Note: This should be #130 in the series, as shown in the table of contents. But p. 288 shows #131. The error was not caught, so the next one in the series is #132. The present article is both #130 and #131.]
Cruickshank, F. R.; Hyde, A. J.; Pugh, D. J. Chem. Educ. 1977, 54, 288.
Thermodynamics
|
A simple lab demonstrating energy transformation Miller, Daniel W.
Building and investigating a sulfuric acid / lead electrolytic cell.
Miller, Daniel W. J. Chem. Educ. 1977, 54, 245.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Thermodynamics
|
Calculators and significant figures Satek, Larry C.
A demonstration on the topic of significant figures and random errors.
Satek, Larry C. J. Chem. Educ. 1977, 54, 177.
Chemometrics
|
What the standard state doesn't say about temperature and phase Carmichael, Halbert
125. The author develops the concept of the "standard state" in a manner that is more robust than typical textbook treatment.
Carmichael, Halbert J. Chem. Educ. 1976, 53, 695.
Thermodynamics |
Phases / Phase Transitions / Diagrams
|
Cookbook dimensional analysis DeLorenzo, Ronald
Frequently, teachers will hear, "...it looks easy when you do it..." when teaching dimensional analysis. This teacher advises others on a way to help students gain self-efficacy with this problem solving-strategy.
DeLorenzo, Ronald J. Chem. Educ. 1976, 53, 633.
Stoichiometry |
Chemometrics
|
A criterion for the simple approximation in dissociation equilibria Leffler, Amos J.
The author demonstrates quantitative criterion for the assumption that permits the neglect of the amount of dissociated species in the denominator of the dissociation equation.
Leffler, Amos J. J. Chem. Educ. 1976, 53, 460.
Acids / Bases |
Equilibrium |
Chemometrics
|
Remembering the sign conventions for q and w in ?E = q - w Gasparro, Francis P.
The author developed a quasi-historical rationalization to help students remember the mathematical statement of the First Law of Thermodynamics.
Gasparro, Francis P. J. Chem. Educ. 1976, 53, 389.
Thermodynamics
|
Freezing ice cream and making caramel topping Plumb, Robert C.; Olson, John Otto; Bowman, Leo H.
The obscurity of "colligative properties" can be dispelled by this ice cream example.
Plumb, Robert C.; Olson, John Otto; Bowman, Leo H. J. Chem. Educ. 1976, 53, 49.
Phases / Phase Transitions / Diagrams |
Physical Properties |
Thermodynamics |
Applications of Chemistry
|
Footnote to the drinking duck exemplum Plumb, Robert C.; Cross, Judson B.; Keil, Robert G.
Variations on the drinking bird demonstration.
Plumb, Robert C.; Cross, Judson B.; Keil, Robert G. J. Chem. Educ. 1975, 52, 728.
Thermodynamics |
Phases / Phase Transitions / Diagrams
|
Questions [and] Answers Campbell, J. A.
203-205. Three chemistry questions and their answers.
Campbell, J. A. J. Chem. Educ. 1975, 52, 587.
Enrichment / Review Materials |
Thermodynamics |
Calorimetry / Thermochemistry
|
A logic diagram for teaching stoichiometry Tyndall, John R.
Presents a diagram that the author found helpful in teaching the fundamentals of stoichiometry.
Tyndall, John R. J. Chem. Educ. 1975, 52, 492.
Stoichiometry |
Chemometrics
|
Maximizing profits in equilibrium processes Rish, Ronald J.
Provides the student with an example in which both chemical principles and calculus are applied to a realistic industrial situation where profits are a must.
Rish, Ronald J. J. Chem. Educ. 1975, 52, 441.
Equilibrium |
Industrial Chemistry |
Chemometrics
|
Brief introduction to the three laws of thermodynamics Stevenson, Kenneth L.
Brief descriptions of the three laws of thermodynamics.
Stevenson, Kenneth L. J. Chem. Educ. 1975, 52, 330.
Thermodynamics
|
Molar solubility calculations and the control equilibrium Chaston, S. H. H.
The Control-Equilibrium method uses as its starting point a precise procedure for obtaining the equilibrium that accounts for the bulk of the decomposition of starting materials.
Chaston, S. H. H. J. Chem. Educ. 1975, 52, 206.
Solutions / Solvents |
Chemometrics |
Equilibrium
|
Illustrating large and small numbers. A problem for the birds Sattler, Louis
A calculation designed to illustrate the relative size of Avogadro's number. The solution from p. 181 is reproduced in this PDF.
Sattler, Louis J. Chem. Educ. 1975, 52, 180.
Chemometrics |
Stoichiometry
|
P-Chem crossword puzzle Snead, Claybourne C.
A physical chemistry crossword puzzle. The answer from p. 174 is reproduced in this PDF.
Snead, Claybourne C. J. Chem. Educ. 1975, 52, 158.
Thermodynamics
|
FeSCN2+ - A computer aid to the CHEM Study experiment McCall, Arthur J., Jr.
A Fortran program assists in making the calculations that accompany investigation of the iron(III)thiocyanate equilibrium system.
McCall, Arthur J., Jr. J. Chem. Educ. 1975, 52, 118.
Equilibrium |
Aqueous Solution Chemistry |
Chemometrics
|
Thermodynamics, folk culture, and poetry Smith, Wayne L.
The principles of the first, second, and third laws of thermodynamics are illustrated in songs and poems.
Smith, Wayne L. J. Chem. Educ. 1975, 52, 97.
Thermodynamics
|
Discussion: Mathematics in the first-year chemistry course Richter, G. P.
Report of the Third Biennial Conference on Chemical Education and the Second Centennial of Chemistry Celebration.
Richter, G. P. J. Chem. Educ. 1975, 52, 19.
Conferences |
Professional Development |
Chemometrics
|
A vigorous, spontaneous endothermic reaction Hawkins, Malcolm D.
Hawkins, Malcolm D. J. Chem. Educ. 1974, 51, A178.
Thermodynamics
|
An endothermic reaction Burt, Norman E.
Burt, Norman E. J. Chem. Educ. 1974, 51, A178.
Thermodynamics
|
Goal-oriented teaching of thermodynamics in general chemistry Canham, G. W. Rayner
Thermodynamics can be more interesting if biological applications are emphasized.
Canham, G. W. Rayner J. Chem. Educ. 1974, 51, 600.
Biophysical Chemistry |
Thermodynamics
|
Computer-enhanced laboratory experience. An example of a totally integrated approach Davis, Leslie N.; Coffey, Charles E.; Macero, Daniel J.
A gas law experiment (Boyle's Law) adapted to make use of computer assisted instruction.
Davis, Leslie N.; Coffey, Charles E.; Macero, Daniel J. J. Chem. Educ. 1973, 50, 711.
Gases |
Thermodynamics
|
A practical energy experiment or lecture demonstration Garin, David L.
Presents two demonstrations: one involves heating different volumes of water on the same heater and measuring their temperatures; the other involves heating different volumes of water on the same heater and calculating the heat of vaporization.
Garin, David L. J. Chem. Educ. 1973, 50, 497.
Calorimetry / Thermochemistry |
Phases / Phase Transitions / Diagrams |
Thermodynamics
|
A computer program for heat of combustion calculations Wilhoit, Randolph C.; Bell, Mary Ellen; Subach, Daniel J.; Chen, Carol
A computer program is available for converting raw combustion data to the standard state energy of combustion.
Wilhoit, Randolph C.; Bell, Mary Ellen; Subach, Daniel J.; Chen, Carol J. Chem. Educ. 1973, 50, 486.
Calorimetry / Thermochemistry |
Chemometrics
|
Scuba diving and the gas laws Cooke, E. D.; Baranowski, Conrad
Three illustrations of physical-chemical principles drawn from scuba diving.
Cooke, E. D.; Baranowski, Conrad J. Chem. Educ. 1973, 50, 425.
Gases |
Applications of Chemistry |
Thermodynamics
|
Footnote to the house heating exemplum Plumb, Robert C.; Campbell, J. A.
Offers a simple proof regarding an earlier column.
Plumb, Robert C.; Campbell, J. A. J. Chem. Educ. 1973, 50, 365.
Thermodynamics |
Gases
|
A quick scored item analysis for objective tests Stokes, Jimmy C.; Strickland, James F., Jr.
Analyzing test data with students in the classroom.
Stokes, Jimmy C.; Strickland, James F., Jr. J. Chem. Educ. 1973, 50, 354.
Chemometrics
|
The first law. For scientists, citizens, poets and philosophers Bent, Henry A.
Practical experiences and phenomena that serve to illustrate the first law of thermodynamics.
Bent, Henry A. J. Chem. Educ. 1973, 50, 323.
Thermodynamics
|
Syphon and the potential energy diagrams Sarbolouki, M. N.
An analogy between the operation of a syphon and potential energy diagrams.
Sarbolouki, M. N. J. Chem. Educ. 1973, 50, 245.
Reactions |
Thermodynamics
|
Physical chemistry of the drinking duck Plumb, Robert C.; Wagner, Robert E.
The operation of the drinking bird is easily understood in terms of a few elementary physical chemistry principles.
Plumb, Robert C.; Wagner, Robert E. J. Chem. Educ. 1973, 50, 213.
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Equilibrium
|
Enthalpy and entropy of evaporation from measured vapor pressure using a programmable desk calculator McEachern, Douglas M.
A program for a calculator that calculates the heat of evaporation of a solid or a liquid and the corresponding entropy change.
McEachern, Douglas M. J. Chem. Educ. 1973, 50, 190.
Calorimetry / Thermochemistry |
Thermodynamics |
Phases / Phase Transitions / Diagrams |
Chemometrics
|
LeChatelier's principle and a rubber band DeLorenzo, Ronald
The cited demonstration can also be sued to illustrate LeChatelier's principle .
DeLorenzo, Ronald J. Chem. Educ. 1973, 50, 124.
Equilibrium |
Thermodynamics
|
Problem solving for chemistry (Peters, Edward I.) Fiekers, Bernard A., S. J.
Fiekers, Bernard A., S. J. J. Chem. Educ. 1972, 49, A491.
Chemometrics
|
Chemical calculations (Benson, Sidney W.) Melgaard, Kennett G.
Melgaard, Kennett G. J. Chem. Educ. 1972, 49, A98.
Chemometrics
|
Questions [and] Answers Campbell, J. A.
Seven questions requiring the application of basic principles of chemistry.
Campbell, J. A. J. Chem. Educ. 1972, 49, 769.
Enrichment / Review Materials |
Applications of Chemistry |
Thermodynamics |
Gases |
Astrochemistry
|
Significant digits in logarithm-antilogarithm interconversions Jones, Donald E.
Most textbooks are in error in the proper use of significant digits when interconverting logarithms and antilogarithms.
Jones, Donald E. J. Chem. Educ. 1972, 49, 753.
Nomenclature / Units / Symbols |
Chemometrics
|
A "relevant" first experiment for freshman chemistry laboratory Macomber, Roger S.
This activity involves popping corn and introduces students to the processes of observation and inference as well as the use of the analytical balance and gravimetric procedure.
Macomber, Roger S. J. Chem. Educ. 1972, 49, 714.
Chemometrics
|
Faster dinner via molecular potential energy Modestino, Sherwood A.
The cooking time for a beef roast can be reduced by using a device that acts as a heat pipe.
Modestino, Sherwood A. J. Chem. Educ. 1972, 49, 706.
Heat Capacity |
Phases / Phase Transitions / Diagrams |
Applications of Chemistry |
Consumer Chemistry
|
Definition of standard states Lukens, David C.
A suggested sequence of definitions for the standard state.
Lukens, David C. J. Chem. Educ. 1972, 49, 654.
Thermodynamics |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Aqueous Solution Chemistry |
Solutions / Solvents
|
An interactive program for teaching pH and logarithms Eskinazi, Jak; Macero, Daniel J.
A computer program written in APL for teaching students logarithms and pH calculations.
Eskinazi, Jak; Macero, Daniel J. J. Chem. Educ. 1972, 49, 571.
pH |
Acids / Bases |
Chemometrics
|
Freezing curves for Salol Laswick, Patty Hall
The convenient freezing temperature of salol (40-43 C) means that students can easily and safely melt the material using warm water
Laswick, Patty Hall J. Chem. Educ. 1972, 49, 537.
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Nonmajor Courses |
Kinetic-Molecular Theory
|
When You Heat Your House Does the Thermal Energy Content Increase? Bilkadi, Zayn; Bridgman, Wilbur B.
Whether or not the total energy content of the air increases or decreases cannot be answered unambiguously.
Bilkadi, Zayn; Bridgman, Wilbur B. J. Chem. Educ. 1972, 49, 493.
Thermodynamics
|
Entropy and a rubber band Laswick, Patty Hall
A temperature change is noted when a rubber band held against the cheek is stretched and then released.
Laswick, Patty Hall J. Chem. Educ. 1972, 49, 469.
Thermodynamics
|
Questions [and] Answers Campbell, J. A.
Five questions requiring an application of basic chemical principles.
Campbell, J. A. J. Chem. Educ. 1972, 49, 328.
Enrichment / Review Materials |
Applications of Chemistry |
Nuclear / Radiochemistry |
Thermodynamics |
Mass Spectrometry |
Isotopes
|
The two-place logarithm table. An aid to understanding and use of logarithms Freiser, Henry
Presents a two-place logarithm table that serves to aid the understanding and use of logarithms.
Freiser, Henry J. Chem. Educ. 1972, 49, 325.
Chemometrics
|
Density of a binary mixture. A classroom or laboratory exercise Feinstein, H. I.
Provides a hypothetical problem in the density of a binary mixture.
Feinstein, H. I. J. Chem. Educ. 1972, 49, 111.
Physical Properties |
Chemometrics
|
Using alligation alternate to solve composition problems Mancott, Anatol
Problems involving the composition of mixtures may be solved by using the relatively obscure method of "alligation alternate" in lieu of the standard algebraic procedure with no loss in accuracy; includes five examples.
Mancott, Anatol J. Chem. Educ. 1972, 49, 57.
Chemometrics |
Solutions / Solvents |
Isotopes
|
The effervescence of ocean surf Plumb, Robert C.; Blanchard, Duncan C.; Bilofsky, Howard S.; Bridgman, Wilbur B.
A pure liquid will not foam, but all true solutions will, as dictated by the fundamental concepts of surface thermodynamics enunciated by Gibbs.
Plumb, Robert C.; Blanchard, Duncan C.; Bilofsky, Howard S.; Bridgman, Wilbur B. J. Chem. Educ. 1972, 49, 29.
Water / Water Chemistry |
Aqueous Solution Chemistry |
Gases |
Solutions / Solvents |
Thermodynamics
|
Entropy Makes Water Run Uphill - in Trees Stevenson, Philip E.
Explains how Sequoias over 300 feet tall can draw water up to their topmost leaves.
Stevenson, Philip E. J. Chem. Educ. 1971, 48, 837.
Applications of Chemistry |
Thermodynamics |
Plant Chemistry |
Membranes |
Transport Properties |
Solutions / Solvents
|
Tire Inflation Thermodynamics Plumb, Robert C.; Connors, John J.
Explains why inflating a tire with a hand pump heats the air being pumped into the tire.
Plumb, Robert C.; Connors, John J. J. Chem. Educ. 1971, 48, 837.
Gases |
Thermodynamics |
Applications of Chemistry
|
Miscellanea No. 6 Eberhardt, W. H.
A collection of clarified, underemphasized, and misunderstood topics, including cell electromotive force and disproportionate reactions; partially miscible liquids and upper consolute temperatures; enthalpy and free energy of formation; and magnetic moment.
Eberhardt, W. H. J. Chem. Educ. 1971, 48, 829.
Electrochemistry |
Solutions / Solvents |
Thermodynamics |
Magnetic Properties
|
Audio taped explanations of freshman experimental calculations Harrison, Aline M.
The authors have found audio tapes to be effective replacements for live, in-lab explanations of experimental calculations.
Harrison, Aline M. J. Chem. Educ. 1971, 48, 826.
Chemometrics |
Laboratory Management
|
SI units in physico-chemical calculations Norris, A. C.
This article demonstrates how the adoption of SI units affects some of the more important physico-chemical calculations found at the undergraduate level.
Norris, A. C. J. Chem. Educ. 1971, 48, 797.
Nomenclature / Units / Symbols |
Chemometrics
|
Heat of hydration Dannhauser, Walter
A commonly published experiment can be expanded so that students may obtain the enthalpy of the reaction between anhydrous salts and water.
Dannhauser, Walter J. Chem. Educ. 1971, 48, 329.
Thermodynamics |
Crystals / Crystallography |
Water / Water Chemistry |
Noncovalent Interactions
|
Acid-base reaction parameters Freiser, Henry
The author demonstrates how the combined algebraic graphical approach can be extended to acid-base titration curve calculations as well as to buffer and sharpness index formulation.
Freiser, Henry J. Chem. Educ. 1970, 47, 809.
Acids / Bases |
pH |
Titration / Volumetric Analysis |
Chemometrics
|
Grading the copper sulfide experiment Novick, Seymour
The author recommends a more liberal analysis in grading the copper sulfide experiment.
Novick, Seymour J. Chem. Educ. 1970, 47, 785.
Stoichiometry |
Chemometrics
|
So-called zeroth law of thermodynamics Redlich, Otto
The "zeroth law of thermodynamics" elucidates the difference between the axiomatic and the epistemological method; it is neither a law nor a statement of fact but a guideline for checking our description of nature.
Redlich, Otto J. Chem. Educ. 1970, 47, 740.
Thermodynamics
|
Chemical exponentialism for beginners Larson, G. Olof
Presents a method for introducing and reviewing exponential mathematical operations.
Larson, G. Olof J. Chem. Educ. 1970, 47, 693.
Chemometrics
|
Culture and the conservation laws Bent, Henry A.
There are no consumers of mass or energy, only converters.
Bent, Henry A. J. Chem. Educ. 1970, 47, 518.
Thermodynamics
|
An alternative to free energy for undergraduate instruction Strong, Laurence E.; Halliwell, H. Frank
It is the purpose of this paper to question the usefulness of the Gibbs function for the student and to propose an alternative based on the use of entropy functions that help the student to focus more sharply on the features of a system that relate to its capacity to change.
Strong, Laurence E.; Halliwell, H. Frank J. Chem. Educ. 1970, 47, 347.
Thermodynamics
|
Our freshmen like the second law Craig, Norman C.
The author affirms the place of thermodynamics in the introductory chemistry course and outlines a presentation that has been used with students at this level.
Craig, Norman C. J. Chem. Educ. 1970, 47, 342.
Thermodynamics
|
The second law - How much, how soon, to how many? Bent, Henry A.
Discussion of the conceptual components of thermodynamics, their mathematical requirements, and where they might be best placed in the curriculum.
Bent, Henry A. J. Chem. Educ. 1970, 47, 337.
Thermodynamics |
Calorimetry / Thermochemistry
|
Sealed tube experiments Campbell, J. A.
Lists and briefly describes a large set of "sealed tube experiments," each of which requires less than five minutes to set-up and clean-up, requires less than five minutes to run, provides dramatic results observable by a large class, and illustrates important chemical concepts.
Campbell, J. A. J. Chem. Educ. 1970, 47, 273.
Thermodynamics |
Crystals / Crystallography |
Solids |
Liquids |
Gases |
Rate Law |
Equilibrium
|
Cloud Caps on High Mountains Stevenson, Philip E.
The formation of cloud caps on high mountains illustrates cooling in an adiabatic expansion and the change in vapor pressure of a liquid with temperature.
Stevenson, Philip E. J. Chem. Educ. 1970, 47, 272.
Atmospheric Chemistry |
Gases |
Applications of Chemistry |
Phases / Phase Transitions / Diagrams |
Thermodynamics
|
The Methanol Lighter Bailar, John C., Jr.
The methanol lighter illustrates the roles that thermodynamics, kinetics, and catalysis play in determining if a reaction will take place.
Bailar, John C., Jr. J. Chem. Educ. 1970, 47, 272.
Thermodynamics |
Kinetics |
Catalysis |
Consumer Chemistry |
Applications of Chemistry
|
The snowmaking machines Plumb, Robert C.
Illustrating principles of thermodynamics in gas expansions and phase changes.
Plumb, Robert C. J. Chem. Educ. 1970, 47, 176.
Gases |
Thermodynamics |
Phases / Phase Transitions / Diagrams
|
Chemical principles exemplified Plumb, Robert C.
Introduction to a new series, containing "exempla" (brief anecdotes about materials and phenomena which exemplify chemical principles). [Debut]
Plumb, Robert C. J. Chem. Educ. 1970, 47, 175.
Gases |
Kinetic-Molecular Theory |
Phases / Phase Transitions / Diagrams |
Thermodynamics |
Equilibrium |
Photochemistry |
Applications of Chemistry
|
Hydrolysis of sodium carbonate Nakayama, F. S.
Presents a procedure for obtaining the ion concentrations of the various component species produced by the hydrolysis of sodium carbonate.
Nakayama, F. S. J. Chem. Educ. 1970, 47, 67.
Aqueous Solution Chemistry |
Chemometrics |
pH
|
Component concentrations in solutions of weak acids Goldish, Dorothy M.
presents a new approach to teaching the subject of weak acid equilibria and its associated calculations.
Goldish, Dorothy M. J. Chem. Educ. 1970, 47, 65.
Acids / Bases |
Aqueous Solution Chemistry |
Equilibrium |
Chemometrics |
pH
|
Essential Math for the Sciences: Algebra, Trigonometry, and Vectors (Beiser, Arthur) Reuland, Donald J.
Reuland, Donald J. J. Chem. Educ. 1969, 46, A899.
Chemometrics
|
Volkswagen versus the hummingbird Nebbia, Giorgio
Questions the cited (046-07-0455) thermodynamic calculations.
Nebbia, Giorgio J. Chem. Educ. 1969, 46, 701.
Thermodynamics |
Calorimetry / Thermochemistry |
Chemometrics
|
LTE. Crocker, Roger
The author points out that the objections raised to his earlier work are academic.
Crocker, Roger J. Chem. Educ. 1969, 46, 699.
Stoichiometry |
Chemometrics
|
LTE. Algebra and chemical equations Copley, George Novello
The author questions the mathematic validity of the cited work.
Copley, George Novello J. Chem. Educ. 1969, 46, 699.
Stoichiometry |
Chemometrics
|
Fuel conversion in transport phenomena Gerlach, E. R.
Calculations comparing the fuel efficiency of a hummingbird with that of a Volkswagen.
Gerlach, E. R. J. Chem. Educ. 1969, 46, 455.
Calorimetry / Thermochemistry |
Chemometrics |
Nomenclature / Units / Symbols
|
A distribution experiment Campbell, J. A.; Nelson, Douglas; Rudesill, John
An experiment to determine the distribution coefficient of an acid between an aqueous and nonaqueous phase.
Campbell, J. A.; Nelson, Douglas; Rudesill, John J. Chem. Educ. 1969, 46, 454.
Acids / Bases |
Aqueous Solution Chemistry |
Thermodynamics |
Equilibrium |
Titration / Volumetric Analysis
|
Indirect calorimetry by computer in the general chemistry course DeMattia, Dennis; Gruhn, Thomas; Gorman, Mel
Describes the use of a Fortran IV program to stimulate student interest in the applications and potential of computer techniques in chemistry.
DeMattia, Dennis; Gruhn, Thomas; Gorman, Mel J. Chem. Educ. 1969, 46, 398.
Calorimetry / Thermochemistry |
Thermodynamics
|
A computer program for the analysis of the N2O4 dissociation equilibrium Erickson, Luther E.
Describes a Fortran IV program for the analysis of empirical data collected for the N2O4 dissociation equilibrium.
Erickson, Luther E. J. Chem. Educ. 1969, 46, 383.
Equilibrium |
Thermodynamics
|
Quantities of work in thermodynamic equations Wright, P. G.
Examines distinctions to be made between work done by forces exerted by external bodies and acting on a system with work done by forces exerted by the system on external bodies.
Wright, P. G. J. Chem. Educ. 1969, 46, 380.
Thermodynamics
|
Thermochemistry of hypochlorite oxidations Bigelow, M. Jerome
Students mix various proportions of aqueous sodium hypochlorite and sodium sulfite and plot the change in temperature to determine the stoichiometry of the reaction.
Bigelow, M. Jerome J. Chem. Educ. 1969, 46, 378.
Calorimetry / Thermochemistry |
Oxidation / Reduction |
Aqueous Solution Chemistry |
Stoichiometry |
Thermodynamics |
Mechanisms of Reactions
|
Chemical queries. Especially for introductory chemistry teachers Young, J. A.; Malik, J. G.
(1) Is there such a thing as a negative pH value? Or one above 14? (2) What is entropy, in terms a beginner may understand? (3) On calculating the molecular weight of a solute from concentration and freezing point depression.
Young, J. A.; Malik, J. G. J. Chem. Educ. 1969, 46, 36.
Acids / Bases |
Aqueous Solution Chemistry |
pH |
Thermodynamics |
Molecular Properties / Structure
|
Circular slide rule conversion of pH to [H+] Grimm, Larry C.
This short note discusses the use of a circular slide rule to convert pH to [H+].
Grimm, Larry C. J. Chem. Educ. 1969, 46, 22.
Chemometrics |
Acids / Bases |
pH |
Aqueous Solution Chemistry
|
Hazardous chemicals data National Fire Protection Association
Explains aspects of chemical hazard data and presents hazards associated with acetaldehyde.
National Fire Protection Association J. Chem. Educ. 1968, 45, A115.
Chemometrics |
Aldehydes / Ketones |
Laboratory Management
|
Why does methane burn? Sanderson, R. T.
A thermodynamic explanation for why methane burns.
Sanderson, R. T. J. Chem. Educ. 1968, 45, 423.
Thermodynamics |
Reactions |
Oxidation / Reduction |
Calorimetry / Thermochemistry |
Covalent Bonding |
Ionic Bonding
|
Energy cycles Haight, G. P., Jr.
Points out limitations and potential pitfalls associated with the use energy cycles to show the atomic and molecular energy factors that may influence an observable chemical property.
Haight, G. P., Jr. J. Chem. Educ. 1968, 45, 420.
Thermodynamics
|
Chemical dynamics for college freshmen Hammond, George S.; Gray, Harry B.
Suggestions for topics regarding chemical dynamics to be considered in freshman chemistry.
Hammond, George S.; Gray, Harry B. J. Chem. Educ. 1968, 45, 354.
Thermodynamics |
Kinetics |
Reactions |
Mechanisms of Reactions |
Rate Law
|
Energy and Entropy in Chemistry (Wyatt, P. A. H.) Strong, Laurence E.
Strong, Laurence E. J. Chem. Educ. 1968, 45, 71.
Thermodynamics
|
Biological oxidations and energy conservation Kirschbaum, Joel
Examines the oxidative steps leading to the synthesis of ATP in living organisms and their metabolic control.
Kirschbaum, Joel J. Chem. Educ. 1968, 45, 28.
Bioenergetics |
Oxidation / Reduction |
Thermodynamics |
Metabolism
|
Energy E. Mechanical Energy Owens, Charles
A steam engine demonstrates the transformation of heat into motion.
Owens, Charles J. Chem. Educ. 1967, 44, A273.
Thermodynamics
|
Chlorine trifluoride. Steere, Norman V.
Summarizes the hazards associated with chlorine trifluoride.
Steere, Norman V. J. Chem. Educ. 1967, 44, A1057.
Chemometrics |
Laboratory Management
|
Letter to the editor Brescia, Frank
Calls on instructors not to confuse students with inappropriate definitions of work.
Brescia, Frank J. Chem. Educ. 1967, 44, 771.
Thermodynamics |
Nomenclature / Units / Symbols
|
A simple analogy of the relationship of ?G to the position of equilibrium Marks, D. J.
This short note describes a simple demonstration to serve as an analogy of the relationship of ?G to the position of equilibrium.
Marks, D. J. J. Chem. Educ. 1967, 44, 402.
Thermodynamics |
Equilibrium
|
The significance of significant figures Pinkerton, Richard C.; Gleit, Chester E.
This paper is an attempt to clarify some of our ideas about numerical data, measurements, mathematical operations, and significant figures.
Pinkerton, Richard C.; Gleit, Chester E. J. Chem. Educ. 1967, 44, 232.
Nomenclature / Units / Symbols |
Chemometrics
|
Textbooks errors. Miscellanea no. 5 Mysels, Karol J.
Considers inconsistencies in the units involved in thermodynamic expressions, incorrect units given for equivalent conductivity, oscillations in polargraphic measurements, and inconsistencies in dealing with catalysis.
Mysels, Karol J. J. Chem. Educ. 1967, 44, 44.
Nomenclature / Units / Symbols |
Thermodynamics |
Catalysis
|
Energy B. Heat energy Hornbeck, Leroy G.; Noerdin, Isjrin; Alyea, Hubert N.
Demonstrations presented include the absorption of black vs white surfaces, the heat ignition of touching flash-bulbs, the low heat of combustion of guncotton, and the heats of displacement of metals.
Hornbeck, Leroy G.; Noerdin, Isjrin; Alyea, Hubert N. J. Chem. Educ. 1966, 43, A978.
Metals |
Thermodynamics
|
Lectures on Matter and Equilibrium (Hill, Terrell L.) Rosenburg, Robert
Rosenburg, Robert J. Chem. Educ. 1966, 43, A1086.
Thermodynamics |
Enrichment / Review Materials
|
The fundamental assumptions of chemical thermodynamics MacRae, Duncan
Examines the fundamental terms, definitions, and assumptions of chemical thermodynamics.
MacRae, Duncan J. Chem. Educ. 1966, 43, 586.
Thermodynamics
|
Demonstrations of spontaneous endothermic reactions Matthews, G. W. J.
The reaction between hydrated metal chlorides and thionyl chloride provides a series of valuable experiments that can be used to demonstrate spontaneous endothermic reactions.
Matthews, G. W. J. J. Chem. Educ. 1966, 43, 476.
Reactions |
Thermodynamics |
Calorimetry / Thermochemistry
|
The enigmatic polymorphism of iron Myers, Clifford E.
Unusual and nontypical, elemental iron can provide the impetus for discussing important chemical principles and properties, including basic thermodynamic concepts and the phenomenon and theory of ferromagnetism.
Myers, Clifford E. J. Chem. Educ. 1966, 43, 303.
Thermodynamics |
Magnetic Properties
|
The use and misuse of the laws of thermodynamics McGlashan, M. L.
Examines the first and second laws, the usefulness of thermodynamics, the calculation of equilibrium constants, and what entropy does not mean.
McGlashan, M. L. J. Chem. Educ. 1966, 43, 226.
Thermodynamics
|
Demonstrating concepts of statistical thermodynamics: More on the Maxwell Demon bottle Sussman, M. V.
The Maxwell Demon bottle can illustrate the nature of entropy, the difference between a work effect and a heat effect, the difference between reversible and irreversible work effects, the mechanical equivalent of heat, and similar intangibles.
Sussman, M. V. J. Chem. Educ. 1966, 43, 105.
Thermodynamics
|
Statistical analysis of data in the general chemistry laboratory Chapin, Earl C.; Burns, Richard F.
Students are asked to analyze data collected with respect to determinations of Dumas molecular weight, equivalent weight of a metal, equivalent weight of an acid, and molecular weight by freezing point depression.
Chapin, Earl C.; Burns, Richard F. J. Chem. Educ. 1965, 42, 564.
Chemometrics
|
Thermodynamics of the ionization of acetic and chloroacetic acids Neidig, H. A., Yingling, R. T.
Students are asked to determine the effect of the structure of acetic, chloroacetic, dichloroacetic, and trichloroacetic acid on equilbria and to discuss the observed effects in terms of standard free energy, enthalpy, and entropy changes.
Neidig, H. A., Yingling, R. T. J. Chem. Educ. 1965, 42, 484.
Acids / Bases |
Thermodynamics |
Aqueous Solution Chemistry
|
Enthalpies of formation of solid salts Neidig, H. A.; Yingling, R. T.
This investigation introduces the student to several important areas of thermochemistry, including enthalpies of neutralization, enthalpies of dissolution, enthalpies of formation, and Hess' Law.
Neidig, H. A.; Yingling, R. T. J. Chem. Educ. 1965, 42, 474.
Thermodynamics |
Solids |
Calorimetry / Thermochemistry |
Precipitation / Solubility |
Acids / Bases |
Aqueous Solution Chemistry
|
Relationship of enthalpy of solution, solvation energy, and crystal energy Neidig, H. A., Yingling, R. T.
The primary objectives of this investigation are to relate enthalpy of solution, solvation energy, and crystal energy using Hess' Law and to acquaint students with Born-Haber type energy cycles.
Neidig, H. A., Yingling, R. T. J. Chem. Educ. 1965, 42, 473.
Thermodynamics |
Solutions / Solvents |
Crystals / Crystallography |
Calorimetry / Thermochemistry
|
Computer program for the calculation of acid-base titration curves Emery, Allan R.
Describes the development of a computer program for the calculation of acid-base titration curves.
Emery, Allan R. J. Chem. Educ. 1965, 42, 131.
Titration / Volumetric Analysis |
Acids / Bases |
Aqueous Solution Chemistry |
Chemometrics
|
Teaching ionic equilibrium: Use of log chart transparencies Freiser, Henry; Fernando, Quintus
The use of graphical methods brings the problem of significance of various terms in complicated expressions into proper focus. Furthermore, a pictorial representation permits the student to see at a glance how the concentrations of various species in a system at equilibrium change with conditions.
Freiser, Henry; Fernando, Quintus J. Chem. Educ. 1965, 42, 35.
Aqueous Solution Chemistry |
Equilibrium |
Acids / Bases |
pH |
Chemometrics |
Brønsted-Lowry Acids / Bases
|
Solubility and pH Calculations (Butler, James N.) Ramette, R. W.
Ramette, R. W. J. Chem. Educ. 1964, 41, A970.
Aqueous Solution Chemistry |
Precipitation / Solubility |
pH |
Acids / Bases |
Chemometrics |
Enrichment / Review Materials
|
Concerning equilibrium, free energy changes, LeChatelier's Principle. III. Halide-halate equilibria Eberhardt, William H.
Compares four equilibria: KI + KIO3, KI + KBrO3, KBR + KBrO3, and KBr + KIO3.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A883.
Equilibrium |
Aqueous Solution Chemistry |
Thermodynamics
|
Concerning equilibrium, free energy changes, Le Châtelier's principle II Eberhardt, William H.
This demonstration involves a reversible, temperature-based transformation from blue tetrahedrally coordinated Co2+ to pink sixfold coordinated Co2+.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A591.
Equilibrium |
Thermodynamics |
Aqueous Solution Chemistry |
Coordination Compounds
|
Problem solving in chemistry (Tilbury, Glen) Whitney, Richard M.
Whitney, Richard M. J. Chem. Educ. 1964, 41, A532.
Chemometrics |
Enrichment / Review Materials
|
Concerning equilibrium, free energy changes, Le Chtelier's principle Eberhardt, William H.
Aqueous KI is added to a solution of CuSO4 in a separatory funnel; adding more CuSO4 demonstrates an equilibrium sift.
Eberhardt, William H. J. Chem. Educ. 1964, 41, A477.
Equilibrium |
Thermodynamics |
Reactions
|
Thermal expansion of gases Barnard, W. Robert
Liquid nitrogen is poured over an inflated balloon.
Barnard, W. Robert J. Chem. Educ. 1964, 41, A139.
Gases |
Thermodynamics |
Kinetic-Molecular Theory
|
Maximum work revisited (Letters) Mysels, Karol J.
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Mysels, Karol J. J. Chem. Educ. 1964, 41, 677.
Thermodynamics |
Gases
|
Maximum work revisited (Letters) Bauman, Robert
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Bauman, Robert J. Chem. Educ. 1964, 41, 676.
Thermodynamics |
Gases
|
Maximum work revisited (Letters) Kokes, Richard J.
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Kokes, Richard J. J. Chem. Educ. 1964, 41, 675.
Thermodynamics |
Gases
|
Maximum work revisited (Letters) Bauman, Robert
Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.
Bauman, Robert J. Chem. Educ. 1964, 41, 675.
Thermodynamics |
Gases
|
Operator formalism in dimensional analysis Musulin, Boris
Describes another approach to dimensional analysis.
Musulin, Boris J. Chem. Educ. 1964, 41, 622.
Chemometrics
|
Reversible and irreversible work: A lecture demonstration Eberhardt, William H.
This lecture demonstration illustrates the concepts of reversible and irreversible work using a pendulum and attached pan balance.
Eberhardt, William H. J. Chem. Educ. 1964, 41, 483.
Thermodynamics
|
The Carnot cycle and Maxwell's relations Nash, Leonard K.
Maxwells equations can be derived from nothing more than the Carnot cycle and the deployment of the simplest plane geometry.
Nash, Leonard K. J. Chem. Educ. 1964, 41, 368.
Thermodynamics |
Chemometrics
|
Beer's law without calculus Pinkerton, Richard C.
There is no good reason for using calculus in the presentation of Beer's law.
Pinkerton, Richard C. J. Chem. Educ. 1964, 41, 366.
Chemometrics
|
Teaching the entropy concept Plumb, Robert C.
Presents a macroscopic lecture demonstration illustrating both potential energy and entropy driving forces and showing their interrelationship.
Plumb, Robert C. J. Chem. Educ. 1964, 41, 254.
Thermodynamics |
Statistical Mechanics
|
A method of visual representation of three dimensional functions Lemlich, Arthur; Zinsser, Hans H.
Lego blocks are used to visually represent three-dimensional functions.
Lemlich, Arthur; Zinsser, Hans H. J. Chem. Educ. 1964, 41, 165.
Chemometrics |
Mathematics / Symbolic Mathematics
|
Work of compressing an ideal gas Bauman, Robert P.
In formulating examples of compression problems there should be an explicit statement that the process is reversible, or at least slow.
Bauman, Robert P. J. Chem. Educ. 1964, 41, 102.
Thermodynamics |
Gases
|
Principles of chemical reaction Sanderson, R. T.
The purpose of this paper is to examine the nature of chemical change in the hope of recognizing and setting forth the basic principles that help us to understand why they occur.
Sanderson, R. T. J. Chem. Educ. 1964, 41, 13.
Reactions |
Thermodynamics |
Mechanisms of Reactions |
Kinetics |
Synthesis |
Covalent Bonding |
Ionic Bonding |
Metallic Bonding
|
An amperometric-kinetic experiment emphasizing the importance of error treatment Young, J. A.
Provides suggestions for student research based on an earlier article published in the Journal.
Young, J. A. J. Chem. Educ. 1963, 40, A139.
Undergraduate Research |
Kinetics |
Chemometrics
|
Chemical calculations (Benson, Sidney W.) Masterton, William L.
Masterton, William L. J. Chem. Educ. 1963, 40, 499.
Chemometrics |
Enrichment / Review Materials
|
Entropy: The significance of the concept of entropy and its applications in science and technology (Fast, J. D.) Bent, Henry A.
Bent, Henry A. J. Chem. Educ. 1963, 40, 442.
Thermodynamics
|
A simple approach to the second law Breck, W. G.
Uses a reversible Carnot cycle as a simple approach to explicating the second law.
Breck, W. G. J. Chem. Educ. 1963, 40, 353.
Thermodynamics
|
Temperature dependence of equilibrium: A first experiment in general chemistry Mahan, Bruce H.
This experiment uses cooling curves to derive the expression for the temperature dependence of the equilibrium constant.
Mahan, Bruce H. J. Chem. Educ. 1963, 40, 293.
Equilibrium |
Thermodynamics
|
Mnemonics for thermodynamic equations Radley, Edward T.; Cohen, Irwin; McCullough, Brother Thomas, C. S. C.
Presents several mnemonics devices for remembering thermodynamic equations.
Radley, Edward T.; Cohen, Irwin; McCullough, Brother Thomas, C. S. C. J. Chem. Educ. 1963, 40, 261.
Thermodynamics
|
Letters to the editor Day, Jesse H.
The author suggests how the importance of thermodynamics might be demonstrated to students.
Day, Jesse H. J. Chem. Educ. 1963, 40, 229.
Thermodynamics
|
Maxwell's demon demonstrator Sussman, M. V.
Describes a simple device used to illustrate the concept of irreversibility.
Sussman, M. V. J. Chem. Educ. 1963, 40, 49.
Thermodynamics
|
Basic mathematics of science and engineering (Wood, Reuben E.) Rosenberg, Robert M.
Rosenberg, Robert M. J. Chem. Educ. 1962, 39, A60.
Chemometrics |
Mathematics / Symbolic Mathematics |
Enrichment / Review Materials
|
Balancing ionic equations by the method of undetermined coefficients Haas, Rudy; Gayer, Karl H.
Describes a mathematical method for balancing chemical equations.
Haas, Rudy; Gayer, Karl H. J. Chem. Educ. 1962, 39, 537.
Stoichiometry |
Chemometrics
|
A second lecture in thermodynamics Burton, Milton
Outlines an introduction for the three laws of thermodynamics
Burton, Milton J. Chem. Educ. 1962, 39, 500.
Thermodynamics
|
The second law of thermodynamics: Introduction for beginners at any level Bent, Henry A.
Examines and offers suggestions for dealing with some of the challenges in teaching thermodynamics at an introductory level.
Bent, Henry A. J. Chem. Educ. 1962, 39, 491.
Thermodynamics
|
Editorially Speaking Kieffer, William F.
Discussion of the conventions, definitions, and symbols of thermodynamics.
Kieffer, William F. J. Chem. Educ. 1962, 39, 489.
Nomenclature / Units / Symbols |
Thermodynamics
|
A simple method for finding slopes Hoare, James P.
Describes a simple method for determining the tangent at any point on a given curve using a solid glass rod.
Hoare, James P. J. Chem. Educ. 1961, 38, 570.
Chemometrics
|
How can you tell whether a reaction will occur? MacWood, George E.; Verhoek, Frank H.
This paper attempts to answer the title question in a clear and direct fashion.
MacWood, George E.; Verhoek, Frank H. J. Chem. Educ. 1961, 38, 334.
Thermodynamics
|
Editorially speaking Kieffer, William F.
Suggests that more should be done to teach introductory college chemistry students basic principles such as entropy and free energy.
Kieffer, William F. J. Chem. Educ. 1961, 38, 333.
Thermodynamics
|
An approach to complex equilibrium problems Butler, James N.
Presents an approach to equilibrium problems that sets up enough equations relating the various concentrations present to define the system completely and then makes approximations that simplify the equations.
Butler, James N. J. Chem. Educ. 1961, 38, 141.
Equilibrium |
Chemometrics |
Acids / Bases |
Aqueous Solution Chemistry
|
A simple ice calorimeter: A first experiment in thermochemistry Mahan, Bruce H.
This note describes a relatively crude and simple ice calorimeter that can be supplied to each student.
Mahan, Bruce H. J. Chem. Educ. 1960, 37, 634.
Calorimetry / Thermochemistry |
Laboratory Equipment / Apparatus |
Thermodynamics
|
Initial ratio of reactants to give, at equilibrium, a maximum yield of products Haslam, E.
Derivation of the initial ratio of reactants to give, at equilibrium, a maximum yield of products.
Haslam, E. J. Chem. Educ. 1958, 35, 471.
Stoichiometry |
Chemometrics
|
An exact titration equation Bolie, Victor W.
The purpose of this paper is to show the development of a titration equation for a precipitation reaction which is exact in the mathematical sense.
Bolie, Victor W. J. Chem. Educ. 1958, 35, 449.
Titration / Volumetric Analysis |
Chemometrics |
Undergraduate Research
|
Radioactive decay calculations without calculus Guenther, William B.
Presents a method for half-life calculations that does not rely on the use of calculus.
Guenther, William B. J. Chem. Educ. 1958, 35, 414.
Chemometrics |
Nuclear / Radiochemistry
|
Solution of problems in chemistry Trousdale, Everett A.
Presents a method for analyzing and solving mole calculations.
Trousdale, Everett A. J. Chem. Educ. 1958, 35, 299.
Chemometrics |
Stoichiometry
|
Dimensional analysis of chemical laws and theories Benfey, O. Theodore
The dimensional analysis of the kinetic theory and organic structural theory.
Benfey, O. Theodore J. Chem. Educ. 1957, 34, 286.
Chemometrics |
Kinetic-Molecular Theory
|
On the second order rate equation Said, Abdel S.
Presents a derivation of the rate equation of a second order reaction.
Said, Abdel S. J. Chem. Educ. 1957, 34, 251.
Kinetics |
Rate Law |
Chemometrics
|
A formula for indirect gravimetry Fiekers, B. A.
Derivation of a formula for indirect gravimetry and application to a sample problem.
Fiekers, B. A. J. Chem. Educ. 1956, 33, 575.
Gravimetric Analysis |
Chemometrics |
Quantitative Analysis
|
A graphical method for determining the order of homogeneous reactions Wright, J. H.; Black, J. H.; Coull, James
Provides a review of classical kinetics, derivation of the reaction order equation, and the determination of reaction order using a graph provided.
Wright, J. H.; Black, J. H.; Coull, James J. Chem. Educ. 1956, 33, 542.
Kinetics |
Chemometrics
|
The experimental determination of an error distribution Nelson, Lloyd S.
Discusses an experiment in which students are asked to the average deviation and probable errors in their measurements.
Nelson, Lloyd S. J. Chem. Educ. 1956, 33, 126.
Chemometrics
|
Why is hydrofluoric acid a weak acid? An answer based on a correlation of free energies, with electronegativities Pauling, Linus
The puzzling behavior of hydrofluoric acid is explained by considering the factors that determine the free energy of hydrogen halogenide molecules and hydrohalogenide ions.
Pauling, Linus J. Chem. Educ. 1956, 33, 16.
Acids / Bases |
Aqueous Solution Chemistry |
Thermodynamics |
Atomic Properties / Structure
|
Pocket slide rule for pH calculations Pitzer, Edgar C.
A pocket slide rule may be used for direct conversion from hydrogen-ion activity to pH, or vice versa, without the need for arithmetical computation.
Pitzer, Edgar C. J. Chem. Educ. 1955, 32, 300.
pH |
Aqueous Solution Chemistry |
Chemometrics
|
Finding the rest point of an undamped analytical balance Stacy, Irving F.
Provides a mathematical analysis for finding the rest point of an undamped analytical balance.
Stacy, Irving F. J. Chem. Educ. 1955, 32, 90.
Laboratory Equipment / Apparatus |
Instrumental Methods |
Chemometrics
|
A general equation for approximate hydronium ion calculations Drenan, James W.
Presents a general equation for simplifying calculations of the hydronium ion.
Drenan, James W. J. Chem. Educ. 1955, 32, 36.
Acids / Bases |
Aqueous Solution Chemistry |
pH |
Chemometrics
|
Proper place problems MacKenzie, Scott
A mathematical analysis of evaluating problems in which students are asked to place items in the correct order.
MacKenzie, Scott J. Chem. Educ. 1954, 31, 428.
Chemometrics
|
A log table for pH problems Condon, Francis E.
Provides a readily remembered log table suitable for computing pH from hydronium-ion concentration and the reverse.
Condon, Francis E. J. Chem. Educ. 1954, 31, 323.
pH |
Chemometrics |
Acids / Bases |
Aqueous Solution Chemistry
|
A heat engine run by rubber Cox, E. G.
Describes a rotating wheel powered by the alternate heating and cooling of rubber bands.
Cox, E. G. J. Chem. Educ. 1954, 31, 307.
Thermodynamics
|
Letters to the editor Weaver, Elbert C.
Acknowledges and corrects an error in the referenced article regarding an example of Pearson's square.
Weaver, Elbert C. J. Chem. Educ. 1954, 31, 102.
Solutions / Solvents |
Chemometrics
|
Letters to the editor Wescott, Emery N.
Points out an error in the referenced article regarding an example of Pearson's square.
Wescott, Emery N. J. Chem. Educ. 1954, 31, 101.
Solutions / Solvents |
Chemometrics
|
Mathematical chemistry Swinbourne, Ellice S.; Lark, P. David
Examines some of the challenges involved in the design of a course in mathematics suitable for undergraduate chemists.
Swinbourne, Ellice S.; Lark, P. David J. Chem. Educ. 1953, 30, 570.
Chemometrics |
Mathematics / Symbolic Mathematics
|
Praseodymium tetrafluoride Perros, Theodore P.; Munson, Thomas R.; Naeser, Charles R.
In spite of the experimental failures to prepare praseodymium tetrafluoride, there is strong evidence for its possible formation to be found by calculating the equilibrium constants for some of the reactions by which this compound might be prepared.
Perros, Theodore P.; Munson, Thomas R.; Naeser, Charles R. J. Chem. Educ. 1953, 30, 402.
Oxidation State |
Equilibrium |
Thermodynamics
|
Letters Angus, L. H.
Suggests a simple temperature-equilibrium demonstration.
Angus, L. H. J. Chem. Educ. 1952, 29, 472.
Thermodynamics
|
A simple demonstration of the Carnot cycle Calingaert, George
This simple demonstration makes use of a stretched rubber band whose temperature changes are noted with the lips.
Calingaert, George J. Chem. Educ. 1952, 29, 405.
Thermodynamics
|
A procedure for solving equilibrium problems Boyd, Robert Neilson
A procedure for solving equilibrium problems is illustrated through several sample problems.
Boyd, Robert Neilson J. Chem. Educ. 1952, 29, 198.
Equilibrium |
Chemometrics |
Aqueous Solution Chemistry
|
A temperature-equilibrium demonstration Brown, John A.
This demonstration makes use of the colored cobaltous complexes in a mixed solvent to show the dependence of some equilibria on temperature.
Brown, John A. J. Chem. Educ. 1951, 28, 640.
Equilibrium |
Calorimetry / Thermochemistry |
Thermodynamics |
Coordination Compounds
|
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