| Journal Articles: 388 results |
|
|
A Dramatic Classroom Demonstration of Limiting Reagent Using the Vinegar and Sodium Hydrogen Carbonate Reaction Romklao Artdej and Tienthong Thongpanchang
This demonstration, appropriate for high school chemistry level and recommended for a large classroom presentation, is designed to illustrate the concept of limiting reagent via a series of experiments in which increasing amounts of sodium bicarbonate are added to a fixed amount of vinegar is fixed until the volume of carbon dioxide generated remains constant.
Artdej, Romklao; Thongpanchang, Tienthong. J. Chem. Educ. 2008, 85, 1382.
Acids / Bases |
Food Science |
Gases |
Stoichiometry
|
Teaching Avogadro's Hypothesis and Helping Students to See the World Differently Brett Criswell
This article uses a model from educational psychologyChi's theory of ontological misclassificationto explain the source of students' difficulties in understanding Avogadro's hypothesis and provide a method to successfully teach this fundamental concept.
Criswell, Brett. J. Chem. Educ. 2008, 85, 1372.
Atomic Properties / Structure |
Gases
|
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
|
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
|
A Hand-Held Ammonia Fountain Nicholas C. Thomas and Stephen Faulk
A plastic juice bottle, filled with ammonia gas generated by combining aqueous ammonia and sodium hydroxide, provides a convenient demonstration of the ammonia fountain and gas solubility.
Thomas, Nicholas C.; Faulk, Stephen. J. Chem. Educ. 2008, 85, 1063.
Aqueous Solution Chemistry |
Gases |
Solutions / Solvents
|
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
|
Similarity and Difference in the Behavior of Gases: An Interactive Demonstration Guy Ashkenazi
A demonstration that concurrently exposes differences and similarities in the behavior of two different gases has been designed to bridge the gap between students' understanding at the algorithmicmacroscopic and conceptualmicroscopic levels.
Ashkenazi, Guy. J. Chem. Educ. 2008, 85, 72.
Gases |
Kinetics |
Learning Theories
|
Effects of a Cooperative Learning Strategy on Teaching and Learning Phases of Matter and One-Component Phase Diagrams Kemal Doymus
Describes a study whose objective was to determine the effects of cooperative learning (using the jigsaw method) on students' achievement in a general chemistry course.
Doymus, Kemal. J. Chem. Educ. 2007, 84, 1857.
Gases |
Liquids |
Phases / Phase Transitions / Diagrams |
Solids
|
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
|
Carbon Dioxide Fountain Seong-Joo Kang and Eun-Hee Ryu
This article presents the development of a carbon dioxide fountain that, unlike the traditional ammonia fountain, is odorless and uses consumer chemicals. This experiment also allows students to see evidence of a gaseous reagent being consumed when a pressure sensor is available.
Kang, Seong-Joo; Ryu, Eun-Hee. J. Chem. Educ. 2007, 84, 1671.
Acids / Bases |
Consumer Chemistry |
Gases |
Laboratory Equipment / Apparatus |
Reactions
|
Incomplete Combustion of Hydrogen: Trapping a Reaction Intermediate Bruce Mattson and Trisha Hoette
In this demonstration, a hydrogen flame is played across the face of an ice cube and the combustion is quenched in an incomplete state. The resulting solution contains a stable side-product, hydrogen peroxide, whose presence can be verified with two simple chemical tests.
Mattson, Bruce; Hoette, Trisha. J. Chem. Educ. 2007, 84, 1668.
Descriptive Chemistry |
Free Radicals |
Gases |
Molecular Properties / Structure |
Reactions |
Reactive Intermediates
|
A Fast Coulometric Estimation of Avogadro's Number Nicholas C. Thomas
Using simple materials found in any high school or college laboratory, an electrochemical method of determining Avogadro's number is presented.
Thomas, Nicholas C. J. Chem. Educ. 2007, 84, 1667.
Electrochemistry |
Gases
|
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
|
Exception to the Le Châtelier Principle Thomas R. Herrinton
Disagreement regarding an apparent exception to the Le Chtelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature.
Herrinton, Thomas R. J. Chem. Educ. 2007, 84, 1427.
Equilibrium |
Gases
|
Exception to the Le Châtelier Principle Thomas R. Herrinton
Disagreement regarding an apparent exception to the Le Chatelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature.
Herrinton, Thomas R. J. Chem. Educ. 2007, 84, 1427.
Equilibrium |
Gases
|
Microscale Demonstration of the Paramagnetism of Liquid Oxygen with a Neodymium Magnet Bruce Mattson
When a neodymium magnet is brought near a suspended glass tube containing a small amount of liquid oxygen, the tube is attracted to the magnet, demonstrating oxygen's paramagnetism. In larger quantities the blue color of liquid oxygen is readily observable.
Mattson, Bruce. J. Chem. Educ. 2007, 84, 1296.
Descriptive Chemistry |
Gases |
Magnetic Properties |
MO Theory |
Molecular Properties / Structure
|
Determining the Pressure inside an Unopened Carbonated Beverage Hans de Grys
Determining the pressure of carbon dioxide inside a sealed soft drink can represents a challenging student exercise. Several methods are discussed for solving the problem, including applying the ideal gas law, gas collection via water displacement, and Henry's law.
de Grys, Hans. J. Chem. Educ. 2007, 84, 1117.
Applications of Chemistry |
Aqueous Solution Chemistry |
Consumer Chemistry |
Food Science |
Gases |
Solutions / Solvents |
Student-Centered Learning
|
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
|
"Concept Learning versus Problem Solving": Does Particle Motion Have an Effect? Michael J. Sanger, Eddie Campbell, Jeremy Felker, and Charles Spencer
210 students were asked to answer a static, particulate-level, multiple-choice question concerning gas properties. Then they viewed an animated version of the question and answered the multiple-choice question again. The distribution of responses changed significantly after students viewed the animation.
Sanger, Michael J.; Campbell, Eddie; Felker, Jeremy; Spencer, Charles. J. Chem. Educ. 2007, 84, 875.
Gases |
Kinetic-Molecular Theory |
Qualitative Analysis |
Quantitative Analysis |
Phases / Phase Transitions / Diagrams
|
What Are Students Thinking When They Pick Their Answer? Michael J. Sanger and Amy J. Phelps
330 students were asked to answer a multiple-choice question concerning gas properties at the microscopic level and explain their reasoning. Of those who selected the correct answer, 80% provided explanations consistent with the scientifically accepted answer, while 90% of the students who picked an incorrect choice provided explanations with at least one misconception.
Sanger, Michael J.; Phelps, Amy J. J. Chem. Educ. 2007, 84, 870.
Gases |
Kinetic-Molecular Theory |
Phases / Phase Transitions / Diagrams |
Qualitative Analysis
|
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
|
The Physical Meaning of the Mathematical Formalism Present in Limiting Chemical Equations; Or, How Dilute Is Dilute? C. Contreras-Ortega, N. Bustamante, J. L. Guevara, C. Portillo, and V. Kesternich
Proposes general mathematical formulations to offer students a better understanding of the real scope of scientific expressions dealing with limiting physical conditions, such as those concerning dilute and concentrated solutions and low and high temperatures and pressures.
Contreras-Ortega, C.; Bustamante, N.; Guevara, J. L.; Portillo, C.; Kesternich, V. J. Chem. Educ. 2007, 84, 788.
Aqueous Solution Chemistry |
Equilibrium |
Gases |
Mathematics / Symbolic Mathematics |
Quantitative Analysis |
Solutions / Solvents
|
Using Dalton's Law of Partial Pressures To Determine the Vapor Pressure of a Volatile Liquid Fred R. Hilgeman, Gary Bertrand, and Brent Wilson
This experiment, designed for a general chemistry laboratory, illustrates the use of Dalton's law of partial pressures to determine the vapor pressure of a volatile liquid.
Hilgeman, Fred R.; Bertrand, Gary; Wilson, Brent. J. Chem. Educ. 2007, 84, 469.
Gases |
Liquids |
Physical Properties |
Solutions / Solvents
|
An Inquiry-Based Chemistry Laboratory Promoting Student Discovery of Gas Laws A. M. R. P. Bopegedera
This article describes a laboratory in which students discover the gas laws using Vernier sensors and Microsoft Excel.
Bopegedera, A. M. R. P. J. Chem. Educ. 2007, 84, 465.
Gases |
Instrumental Methods |
Physical Properties
|
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
|
Where Did the Water Go? Boyle's Law and Pressurized Diaphragm Water Tanks James Brimhall and Sundar Naga
Boyles law (PV is constant) provides mathematical insight into the workings of pressurized diaphragm tanks for storage of water pumped from underground wells, including predictions of the quantities of available water resulting from different initial conditions of water tank systems.
Brimhall, James; Naga, Sundar. J. Chem. Educ. 2007, 84, 425.
Applications of Chemistry |
Gases
|
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
|
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
|
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
|
Chemistry of Electronic Gases James R. Clark
The chemistry of electronic gases can be used in the classroom to provide many interesting examples of molecular structures, chemical reactions, periodic trends, and environmental chemistry.
Clark, James R. J. Chem. Educ. 2006, 83, 857.
Applications of Chemistry |
Gases |
Industrial Chemistry |
Semiconductors |
Solid State Chemistry
|
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
|
General Education and General Chemistry—Redux Leslie S. Forster
This paper discusses the desirability of including non-technical general education topics in chemistry courses intended for science and engineering students.
Forster, Leslie S. J. Chem. Educ. 2006, 83, 614.
Enrichment / Review Materials |
Gases |
Learning Theories
|
The Ultrasonic Soda Fountain: A Dramatic Demonstration of Gas Solubility in Aqueous Solutions John E. Baur and Melinda B. Baur
An ultrasonic bath is used to accelerate the rate at which carbonated beverages equilibrate with the atmosphere. The resulting fountain, which can reach heights in excess of 3 meters, is a dramatic demonstration of the solubility of gases in liquids.
Baur, John E.; Baur, Melinda B. J. Chem. Educ. 2006, 83, 577.
Aqueous Solution Chemistry |
Kinetics |
Physical Properties |
Solutions / Solvents |
Precipitation / Solubility
|
Steel Wool and Oxygen: How Constant Should a Rate Constant Be? Michiel Vogelezang
In the article Steel Wool and Oxygen: A Look at Kinetics, James Gordon and Katherine Chancey describe an experiment about the kinetics between iron and oxygen. Like all good experiments this one is easy to carry out and produces good results. However, the experiment can even have a greater impact with only a small addition.
Vogelezang, Michiel. J. Chem. Educ. 2006, 83, 214.
Rate Law |
Kinetics |
Oxidation / Reduction
|
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
|
Gas Permeability of Polymers Jee-Yon Lee
Undergraduate students can learn what causes the helium-inflated balloon to fall in a few days through the proposed experiment.
Lee, Jee-Yon. J. Chem. Educ. 2005, 82, 1472.
Gases |
Transport Properties
|
Gas Permeability of Polymers Bruno Lunelli
The recent article, Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated Balloon, proposes a model of permeation untenable and in contradiction with correct statements present in the same text and consequently does not consider the material of which the investigated balloons are made.
Lunelli, Bruno. J. Chem. Educ. 2005, 82, 1471.
Gases |
Transport Properties
|
Gas Permeability of Polymers Bruno Lunelli
By studying a number of soft drinks with color but with or without phosphoric acid, the authors have determined that the required 20-fold dilution required in the Determination of Phosphorus in Cola Drinks is not to dilute the color but merely to place the sample within the calibration range of the analysis.
Lunelli, Bruno. J. Chem. Educ. 2005, 82, 1471.
UV-Vis Spectroscopy |
Instrumental Methods |
Gases |
Transport Properties
|
The Fizz-Keeper: A Useful Science Tool John P. Williams, Sandy Van Natta, and Rebecca Knipp
The Fizz-Keeper is well suited for a great variety of pressure-based activities.
Williams, John P.; Van Natta, Sandy; Knipp, Rebecca. J. Chem. Educ. 2005, 82, 1454.
Applications of Chemistry |
Colloids |
Gases
|
Balloon—Toy of Many Colors Kathryn R. Williams
Balloon-related articles previously published in JCE describe gas law experiments and demonstrations, large-scale molecular models, demonstrations of reaction rates and stoichiometry, hydrogen-filled balloon explosions, and miscellaneous laboratory uses.
Williams, Kathryn R. J. Chem. Educ. 2005, 82, 1448.
Gases |
Laboratory Equipment / Apparatus |
VSEPR Theory
|
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
|
Some Insights Regarding a Popular Introductory Gas Law Experiment Ed DePierro and Fred Garafalo
This paper alerts readers to a potential source of error in one approach to the Dumas method as it is often practiced in introductory chemistry laboratories. The room-temperature vapor pressures of volatile compounds that might be considered as unknowns for the experiment lead to determined molar masses that are too low. The greater the vapor pressure of the compound, the lower the determined molar mass will be, when compared to the accepted value.
DePierro, Ed; Garafalo, Fred. J. Chem. Educ. 2005, 82, 1194.
Gases |
Laboratory Equipment / Apparatus |
Phases / Phase Transitions / Diagrams |
Physical Properties
|
Steel Wool and Oxygen: A Look at Kinetics James Gordon and Katherine Chancey
An experimental method is described to study the kinetics of the reaction of the iron in steel wool with molecular oxygen. A calculator-based data collection system is used with an oxygen gas sensor to determine the order of the reaction with respect to oxygen. Using the graphical method, students determine that the reaction follows first-order kinetics with respect to oxygen.
Gordon, James; Chancey, Katherine. J. Chem. Educ. 2005, 82, 1065.
Atmospheric Chemistry |
Gases |
Kinetics |
Oxidation / Reduction
|
Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated Balloon Jee-Yon Lee, Hee-Soo Yoo, Jong Sook Park, Kwang-Jin Hwang, and Jin Seog Kim
In developing this laboratory, our initial motivation for the analysis of gases in a balloon was to answer simple and basic questions, such as, Why does a helium-charged balloon left in the air always drop in a few days? Is leakage of helium the only cause of the drop? What is the composition of the gas in the balloon when it falls after deflation? Students were intrigued by these questions, too, as they analyzed the variation over time in the composition in a balloon inflated with helium. Using the concepts of partial pressure and chemical potential, the laboratory experiment described effectively investigates the diffusion process and the behavior of gas molecules for teaching these concepts in general and physical chemistry.
Lee, Jee-Yon; Yoo, Hee-Soo; Park, Jong Sook; Hwang, Kwang-Jin; Kim, Jin Seog. J. Chem. Educ. 2005, 82, 288.
Transport Properties |
Gases |
Mass Spectrometry |
Quantitative Analysis
|
The Determination of the Percent of Oxygen in Air Using a Gas Pressure Sensor James Gordon and Katherine Chancey
A new detection method is applied to a classic experiment in which gaseous atmospheric oxygen in a test tube is reacted with the iron in steel wool to produce rust. A gas pressure sensor interfaced to a calculator-based data collection system was used to measure the percent of oxygen in the air as the reaction proceeded. The results from the calculator-based experiment were compared to the results from a more traditional water-measurement experiment. The average percent of oxygen obtained using the calculator system was 19.4 0.4%.
Gordon, James; Chancey, Katherine. J. Chem. Educ. 2005, 82, 286.
Atmospheric Chemistry |
Gases |
Oxidation / Reduction |
Reactions
|
Fractional Distillation of Air and Other Demonstrations with Condensed Gases Maria Oliver-Hoyo and William L. Switzer, III
This demonstration builds upon the commonly performed liquefaction of air not only to show the presence of nitrogen and oxygen, but also the presence of two other components, carbon dioxide and water. Several extensions are suggested: one to show boiling point elevation in solution and another to show the elevation of both boiling point and sublimation point with pressure. No special apparatus is required permitting presentations to audiences in a variety of settings. These demonstrations give the opportunity to discuss properties of gases, solution chemistry, and phase equilibria.
Oliver-Hoyo, Maria; Switzer, William L., III. J. Chem. Educ. 2005, 82, 251.
Gases |
Qualitative Analysis |
Atmospheric Chemistry |
Phases / Phase Transitions / Diagrams |
Separation Science
|
A Methane Balloon Inflation Chamber Curtis J. Czerwinski and Tanya J. Cordes
While several lecture demonstrations are possible using methane-filled balloons, it is often inconvenient to prepare these balloons since the pressure from standard laboratory and lecture hall gas nozzles is too low. As a solution to this problem, a methane balloon inflation chamber, prepared from a translucent 3.5-gallon pail and an aspirator or house-vacuum, provides an inexpensive and convenient method for inflating balloons in laboratories or lecture halls. Prepared in this way, methane-filled balloons can be used to demonstrate the effects of vacuum, the lifting power of low-density gases, and the explosive combustion of methane.
Czerwinski, Curtis J.; Cordes, Tanya J. J. Chem. Educ. 2005, 82, 248.
Alkanes / Cycloalkanes |
Calorimetry / Thermochemistry |
Gases |
Oxidation / Reduction |
Reactions
|
On the Buoyancy of a Helium-Filled Balloon John E. Harriman
It is shown by expansion of the exponential in the barometric formula that the forces due to pressure acting on a balloon are of the form (PV/RT)Mg and that results agree with those suggested by Archimedes principle. Einstein's equivalence principal provides an answer to what balloons will do in an accelerated car.
Harriman, John E. J. Chem. Educ. 2005, 82, 246.
Atmospheric Chemistry |
Gases |
Kinetic-Molecular Theory |
Physical Properties
|
Using Clinical Cases To Teach General Chemistry Brahmadeo Dewprashad, Charles Kosky, Geraldine S. Vaz, and Charlotte L. Martin
This article describes how a fact-based clinical case was effectively used to motivate and enrich the classroom experience and review many of the concepts covered in general chemistry. The case involves an elderly patient who was brought to the emergency room. The results of his physical examination and laboratory analysis of his blood are presented. The students, in peer-led groups, work through the chemical principles involved in the doctor's diagnosis and treatment options for the patient. The article describes the case study, instructors' observations, and students' perception of the activity.
Dewprashad, Brahmadeo; Kosky, Charles; Vaz, Geraldine S.; Martin, Charlotte L. J. Chem. Educ. 2004, 81, 1471.
Acids / Bases |
Drugs / Pharmaceuticals |
Equilibrium |
Kinetics |
Medicinal Chemistry
|
Water in the Atmosphere Joel M. Kauffman
None of eight college-level general chemistry texts gave a mean value for water in the atmosphere, despite its being the third most prevalent constituent at about 1.5% by mass as vapor and about 2% if clouds and ice crystals are included. The importance of water as a greenhouse gas was omitted or marginalized by five of the eight texts. An infrared spectrum of humid air was determined to demonstrate that water vapor, because of its higher concentration, was more absorptive than carbon dioxide. The cooling effect of clouds, or other influences on the Earth's albedo, were not mentioned in most of the texts. These pervasive errors should be corrected in new or future editions of textbooks.
Kauffman, Joel M. J. Chem. Educ. 2004, 81, 1229.
Atmospheric Chemistry |
Gases |
Green Chemistry |
IR Spectroscopy
|
Using a Datalogger To Determine First-Order Kinetics and Calcium Carbonate in Eggshells Martin M. F. Choi and Pui Shan Wong
The purpose of this article is to demonstrate the use of a datalogger in conjunction with a pressure sensor to monitor the generation of carbon dioxide when calcium carbonate is in contact with hydrochloric acid.
Choi, Martin M. F.; Wong, Pui Shan. J. Chem. Educ. 2004, 81, 859.
Kinetics |
Food Science |
Microscale Lab |
Quantitative Analysis |
Laboratory Computing / Interfacing
|
Kinetics of the Osmotic Hydration of Chickpeas Gabriel Pinto and Ali Esin
An experiment examining the swelling of chickpeas as they are soaked in water is presented to introduce students to topics such as osmotic flow, mass transfer, diffusion, kinetics of hydration, modeling, and estimation of activation energy.
Pinto, Gabriel; Esin, Ali. J. Chem. Educ. 2004, 81, 532.
Kinetics |
Water / Water Chemistry |
Food Science |
Transport Properties
|
Chemistry and Song: A Novel Way To Educate and Entertain Cory C. Pye
In this article, a novel way of teaching chemistry is presented that uses contemporary music and chemical lyrics to educate.
Pye, Cory C. J. Chem. Educ. 2004, 81, 507.
Gases
|
Bringing History to the Classroom: Spoofs about Problems in Obtaining Research Grants Sidney Toby
This article is a spoof on the History of Science and consists of four skits depicting the difficulties famous men and women in science might have had in fictional interviews while seeking funding for their research.
Toby, Sidney. J. Chem. Educ. 2004, 81, 503.
Gases |
Physical Properties |
Nuclear / Radiochemistry |
Women in Chemistry |
Administrative Issues
|
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
|
The Decomposition of Zinc Carbonate: Using Stoichiometry To Choose between Chemical Formulas Stephen DeMeo
To determine which formula corresponds to a bottle labeled "zinc carbonate", students perform qualitative tests on three of zinc carbonate's decomposition products: zinc oxide, carbon dioxide, and water. Next students make quantitative measurements to find molar ratios and compare them with the coefficients of the balanced chemical equations. This allows the correct formula of zinc carbonate to be deduced.
DeMeo, Stephen. J. Chem. Educ. 2004, 81, 119.
Gases |
Stoichiometry |
Quantitative Analysis
|
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
|
Carbon Dioxide Flooding: A Classroom Case Study Derived from Surgical Practice Robert C. Kerber
The surgical opening in open-heart surgery is often flooded with carbon dioxide gas to avoid air embolisms when the heart is closed and restarted. This practice can be used in chemistry courses to illustrate concepts of gas density, solubility, and acidbase equilibria, including buffering.
Kerber, Robert C. . J. Chem. Educ. 2003, 80, 1437.
Acids / Bases |
Aqueous Solution Chemistry |
Gases |
Medicinal Chemistry |
Nonmajor Courses |
Applications of Chemistry
|
Why Does a Helium-Filled Balloon "Rise"? Richard W. Ramette
The article is a lighthearted, conversational exploration of the microscopic basis for Archimedes principle. The principle is discussed in terms of molecular collisions and density gradients in a gravitational field.
Ramette, Richard W. J. Chem. Educ. 2003, 80, 1149.
Atmospheric Chemistry |
Gases |
Kinetic-Molecular Theory |
Physical Properties
|
Decomposition Kinetics of Hydrogen Peroxide: Novel Lab Experiments Employing Computer Technology Dorota A. Abramovitch, Latrice K. Cunningham, and Mitchell R. Litwer
Using a sensor to measure changes in the pressure of oxygen produced by the decomposition of hydrogen peroxide as a means of analyzing this reaction and factors that affect its rate.
Abramovitch, Dorota A.; Cunningham, Latrice K.; Litwer, Mitchell R. J. Chem. Educ. 2003, 80, 790.
Gases |
Laboratory Computing / Interfacing |
Kinetics
|
Kinetics of Platinum-Catalyzed Decomposition of Hydrogen Peroxide Tiffany A. Vetter and D. Philip Colombo Jr.
Determining the order and rate constant of the catalyzed decomposition of hydrogen peroxide using AOSEPT contact lens cleaning and a platinum-coated AOSEPT disc.
Vetter, Tiffany A.; Colombo, D. Philip, Jr. J. Chem. Educ. 2003, 80, 788.
Catalysis |
Consumer Chemistry |
Kinetics |
Laboratory Computing / Interfacing |
Rate Law
|
The Universal Gas Constant R William B. Jensen
Answers the question "Why is the universal gas constant represented by the letter R?" [Debut]
Jensen, William B. J. Chem. Educ. 2003, 80, 731.
Gases |
Enrichment / Review Materials
|
Applying the Reaction Table Method for Chemical Reaction Problems (Stoichiometry and Equilibrium) Steven F. Watkins
A systematic approach to chemical reaction calculations (stoichiometry calculations) - the "Reaction Table Method" (similar to the equilibrium table method).
Watkins, Steven F. J. Chem. Educ. 2003, 80, 658.
Equilibrium |
Stoichiometry |
Reactions |
Kinetics
|
Bubble Stripping To Determine Hydrogen Concentrations in Ground Water: A Practical Application of Henry's Law Daniel M. McInnes and Don Kampbell
Applying Henry's law to determine the concentration of hydrogen in ground water as a means of identifying possible contamination by chlorinated organic compounds.
McInnes, Daniel M.; Kampbell, Don. J. Chem. Educ. 2003, 80, 516.
Water / Water Chemistry |
Gases |
Quantitative Analysis |
Applications of Chemistry
|
Stoichiometry of the Reaction of Magnesium with Hydrochloric Acid Venkat Chebolu and Barbara C. Storandt
Using a pressure sensor to measure the production of hydrogen by a reaction between magnesium and hydrochloric acid.
Chebolu, Venkat; Storandt, Barbara C. J. Chem. Educ. 2003, 80, 305.
Stoichiometry |
Gases |
Laboratory Equipment / Apparatus |
Laboratory Computing / Interfacing |
Reactions
|
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
|
A Novel Microscale Gas Generator Jinhua Wang, Zaisheng Lu, and Changcun Zhao
Design of a microscale gas generator.
Wang, Jinhua; Lu, Zaisheng; Zhao, Changcun. J. Chem. Educ. 2003, 80, 181.
Gases |
Laboratory Equipment / Apparatus |
Microscale Lab
|
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
|
Unknown Gases: Student-Designed Experiments in the Introductory Laboratory John Hanson and Tim Hoyt
Investigation in which students must determine the identity of three unknown gases by developing their own tests.
Hanson, John; Hoyt, Tim. J. Chem. Educ. 2002, 79, 845.
Gases |
Qualitative Analysis |
Physical Properties
|
A Simple Experiment for the Determination of Molecular Weights of Gases Lighter Than Air Van T. Lieu and Gene E. Kalbus
A simple method for the determination of molecular weights of gases lighter than air.
Lieu, Van T.; Kalbus, Gene E. J. Chem. Educ. 2002, 79, 473.
Gases |
Molecular Properties / Structure |
Physical Properties
|
Just Breathe: The Oxygen Content of Air JCE Editorial Staff
Students estimate the percent oxygen (volume) in air using steel wool in a test tube that is inverted in a beaker of water. Oxygen in the trapped air reacts with iron to form rust, and the water level rises inside the test tube; within 30-45 minutes, the majority of oxygen is consumed.
JCE Editorial Staff. J. Chem. Educ. 2001, 78, 512A.
Electrochemistry |
Gases |
Oxidation / Reduction
|
Sink or Swim: The Cartesian Diver K. David Pinkerton
Cartesian divers are a quick and simple way to illustrate relationships among pressure, volume, temperature, and buoyancy. The Activity could be used in connection with the concepts of gases and liquids and discussions of Boyle's, Charles's, and the ideal gas laws.
Pinkerton, K. David. J. Chem. Educ. 2001, 78, 200A.
Gases |
Physical Properties
|
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
|
Determination of the Universal Gas Constant, R. A Discovery Laboratory David B. Moss and Kathleen Cornely
Discovery laboratory in which groups of students collect oxygen, hydrogen, and nitrogen gas over water and determine the value of the universal gas constant, R, using the ideal gas law.
Moss, David B.; Cornely, Kathleen. J. Chem. Educ. 2001, 78, 1260.
Gases
|
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
|
Are Fizzing Drinks Boiling? A Chemical Insight from Chemical Education Research Alan Goodwin
The suggestion that fizzing drinks are examples of liquids boiling at room temperature has proved to be controversial among both chemists and chemical educators. This paper presents a case for believing this everyday system to be a good example of a boiling solution and the consequent separation of carbon dioxide from the solution to exemplify fractional distillation.
Goodwin, Alan. J. Chem. Educ. 2001, 78, 385.
Aqueous Solution Chemistry |
Kinetic-Molecular Theory |
Equilibrium |
Gases |
Solutions / Solvents |
Phases / Phase Transitions / Diagrams
|
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
|
The State of Division of Solids and Chemical Equilibria João C. M. Paiva and Victor M. S. Gil
An experiment and a computer simulation are presented to address a counterintuitive situation often encountered when teaching chemical equilibria. This is prompted by the question "How can the subdivision of a solid reactant affect the reaction rate and not the composition of the equilibrium state?"
Paiva, João C. M.; Gil, Victor M. S. J. Chem. Educ. 2001, 78, 222.
Equilibrium |
Kinetics |
Laboratory Computing / Interfacing
|
JCE Classroom Activity: Out of "Thin Air": Exploring Phase Changes John J. Vollmer
This Activity illustrates sublimation/deposition with para-dichlorobenzene (mothballs) and evaporation/condensation with water.
Vollmer, John J. J. Chem. Educ. 2000, 77, 488A.
Phases / Phase Transitions / Diagrams |
Crystals / Crystallography |
Physical Properties |
Solids |
Gases
|
Using a Computer Animation to Improve Students' Conceptual Understanding of a Can-Crushing Demonstration Michael J. Sanger, Amy J. Phelps, and Jason Fienhold
This paper reports some of the misconceptions that were identified from these students' explanations. As a result of these misconceptions, a computer animation depicting the chemical processes occurring in the can-crushing demonstration was created.
Sanger, Michael J.; Phelps, Amy J.; Fienhold, Jason. J. Chem. Educ. 2000, 77, 1517.
Kinetic-Molecular Theory |
Gases
|
Combustion Demonstration Using Updated Flame Tornado Edward G. Senkbeil
This demonstration uses the combustion of different forms of cellulose and an updated version of the "flame tornado" as an ignition source to illustrate the factors affecting the combustion process. The objectives of the experiment are to illustrate the factors affecting the rate of a combustion reaction and to demonstrate the factors affecting the production of a flame by using the flame tornado.
Senkbeil, Edward G. J. Chem. Educ. 2000, 77, 1449.
Descriptive Chemistry |
Oxidation / Reduction |
Reactions |
Rate Law
|
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
|
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
|
Potentiometric Determination of CO2 Concentration in the Gaseous Phase: Applications in Different Laboratory Activities Eduardo Cortón, Santiago Kocmur, Liliana Haim, and Lydia Galagovsky
The first lab comprises the calibration of a CO2 potentiometric detector with gas mixtures. The CO2 and CO2-free air required for the gaseous samples are produced in the lab by an inexpensive and simple apparatus. In the second lab, the CO2 potentiometric device is used to measure CO2 uptake and release during different metabolic processes.
Cortón, Eduardo; Kocmur, Santiago; Haim, Liliana; Galagovsky, Lydia. J. Chem. Educ. 2000, 77, 1188.
Electrochemistry |
Gases |
Quantitative Analysis |
Metabolism
|
A New Approach to Teaching Introductory Science: The Gas Module Pamela Mills, William V. Sweeney, Robert Marino, and Sandra Clarkson
A lecture/laboratory module about the behavior of gases that is designed to expose students to the process of scientific discovery, not to teach the gas laws per se. The topic of gases is only the medium used to illustrate other important aspects of physical science: how to process experimental data and reduce it to symbolic mathematical relationships, how to evaluate the reliability of experimental data, and how to view the relationship between experimental data and scientific models.
Mills, Pamela A.; Sweeney, William V.; Marino, Robert; Clarkson, Sandra. J. Chem. Educ. 2000, 77, 1161.
Gases
|
Every Year Begins a Millennium Jerry A. Bell
This article outlines a series of demonstrations and their contexts, leading to recommendations about what we teach and how we teach.
Bell, Jerry A. J. Chem. Educ. 2000, 77, 1098.
Acids / Bases |
Aqueous Solution Chemistry |
Equilibrium |
Kinetics |
Learning Theories
|
Paradoxes, Puzzles, and Pitfalls of Incomplete Combustion Demonstrations Ed Vitz
Paper is burned in a closed container containing sufficient oxygen to consume all the paper. Paradoxically, the flame expires while half of the paper remains. This demonstrates that thermodynamics or stoichiometry is insufficient to explain everyday chemical processes, and that kinetics is often necessary. The gases in the container are analyzed by GC before and after combustion, and the results are examined in detail.
Vitz, Ed. J. Chem. Educ. 2000, 77, 1011.
Gases |
Kinetics |
Stoichiometry
|
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
|
Determination of the Fundamental Electronic Charge via the Electrolysis of Water Brittany Hoffman, Elizabeth Mitchell, Petra Roulhac, Marc Thomes, and Vincent M. Stumpo
In an illuminating experiment suitable for secondary school students, a Hoffman electrolysis apparatus is employed to determine the fundamental electronic charge. The volume and pressure of hydrogen gas produced via the electrolysis of water during a given time interval are measured.
Hoffman, Brittany; Mitchell, Elizabeth; Roulhac, Petra; Thomes, Marc; Stumpo, Vincent M. J. Chem. Educ. 2000, 77, 95.
Atomic Properties / Structure |
Electrochemistry |
Gases |
Molecular Properties / Structure
|
Henry's Law and Noisy Knuckles Doris R. Kimbrough
Presented here is the application of Henry's law to the noise associated with "cracking" knuckles. Gases dissolved in the synovial fluid in joints rapidly come out of solution as the joint is stretched and pressure is decreased. This "cavitation" produces a characteristic noise.
Kimbrough, Doris R. J. Chem. Educ. 1999, 76, 1509.
Gases |
Solutions / Solvents |
Applications of Chemistry |
Medicinal Chemistry
|
An Inexpensive Microscale Method for Measuring Vapor Pressure, Associated Thermodynamic Variables, and Molecular Weight Jason C. DeMuro, Hovanes Margarian, Artavan Mkhikian, Kwang Hi No, and Andrew R. Peterson
Existing methods for measuring vapor pressure are too expensive or not quantitative enough for chemistry classes in secondary schools. Our method measures the vapor pressure inside a bubble trapped in a graduated microtube made from a disposable 1-mL glass pipet.
DeMuro, Jason C.; Margarian, Hovanes; Mkhikian, Artavan; No, Kwang Hi; Peterson, Andrew R. J. Chem. Educ. 1999, 76, 1113.
Aqueous Solution Chemistry |
Gases |
Microscale Lab |
Phases / Phase Transitions / Diagrams
|
Variations on the "Whoosh" Bottle Alcohol Explosion Demonstration Including Safety Notes John J. Fortman, Andrea C. Rush, and Jennifer E. Stamper
The explosion or burning of methanol, ethanol, n-propanol, and isopropanol in large small-necked bottles when ignited with a match has been studied with respect to the nature of the alcohol, temperature, concentration dilutions with water, oxygen concentration, plastic versus glass bottles, and salts added for color.
Fortman, John J.; Rush, Andrea C.; Stamper, Jennifer E. J. Chem. Educ. 1999, 76, 1092.
Gases |
Alcohols
|
Relative Humidity R. Bruce Martin
Daily we hear reports of relative humidity, yet most students remain unfamiliar with its import. This short article defines and describes the concept at several levels. A new, general interest, isobaric plot directly indicates the dependence of relative humidity on temperature.
Martin, R. Bruce. J. Chem. Educ. 1999, 76, 1081.
Consumer Chemistry |
Gases |
Nonmajor Courses |
Water / Water Chemistry |
Atmospheric Chemistry
|
A More Dramatic Container to Crush by Atmospheric Pressure Robert D. Meyers and Gordon T. Yee
The familiar demonstration of collapsing a can by filling it with water vapor and then sealing it and allowing it to cool is improved by performing it with a 20-L steel solvent drum instead.
Meyers, Robert D.; Yee, Gordon T. J. Chem. Educ. 1999, 76, 933.
Gases |
Phases / Phase Transitions / Diagrams
|
Ammonia Can Crush Ed Vitz
When a 12-oz aluminum soft drink can filled with ammonia or hydrogen chloride gas is inverted and dipped into water, the rapidly dissolving gas evacuates the can and the can is crushed before water can be drawn into it. This demonstrates, among other things, the remarkable strength of hydrogen bonds.
Vitz, Ed. J. Chem. Educ. 1999, 76, 932.
Noncovalent Interactions |
Gases |
Solutions / Solvents |
Hydrogen Bonding
|
The Persistence of the Candle-and-Cylinder Misconception James P. Birk and Anton E. Lawson
There is a persistent misconception that when a lighted candle is supported in a container of water and a closed cylinder is lowered over the candle, the candle is extinguished after a time by complete consumption of the oxygen in the cylinder, with a volume change corresponding to the amount of oxygen in the air. This misconception has appeared in the literature periodically for many years. Here, we present a number of experiments that refute this misconception.
Birk, James P.; Lawson, Anton E. J. Chem. Educ. 1999, 76, 914.
Gases |
Atmospheric Chemistry |
Quantitative Analysis |
Reactions
|
Equilibrium: A Teaching/Learning Activity (author's reply) Wilson, Audrey
Thanks for clarification and suggestions.
Wilson, Audrey J. Chem. Educ. 1999, 76, 900.
Equilibrium |
Rate Law
|
Equilibrium: A Teaching/Learning Activity Sadavoy, Lyle; Paiva, Joao C. M.; Gil, Victor M. S.
Clarification and suggestions for improvement.
Sadavoy, Lyle; Paiva, Joao C. M.; Gil, Victor M. S. J. Chem. Educ. 1999, 76, 900.
Equilibrium |
Rate Law
|
The Arrhenius Equation Revisited (author's reply) Carroll, Harvey F.
Misleading remarks regarding the Arrhenius equation in some general chemistry texts.
Carroll, Harvey F. J. Chem. Educ. 1999, 76, 899.
Equilibrium |
Rate Law
|
The Arrhenius Equation Revisited Logan, S. R.
Addition citation on the implications of the Arrhenius equation.
Logan, S. R. J. Chem. Educ. 1999, 76, 899.
Equilibrium |
Rate Law
|
The Methane Balloon Walter H. Corkern and Elvin Hughes Jr.
The objectives are (i) to describe a novel method of inflating a balloon with methane, (ii) to show that methane is lighter than air, and (iii) to demonstrate the flammability of methane.
Corkern, Walter H.; Hughes, Elvin, Jr. J. Chem. Educ. 1999, 76, 794.
Gases |
Oxidation / Reduction |
Reactions
|
Pressure and Stoichiometry Charles E. Roser and Catherine L. McCluskey
This experiment determines the stoichiometry of the reaction of a carbonate or hydrogen carbonate and HCl by measuring the pressure of the CO2 produced using a Vernier pressure sensor, TI CBL interface, and a TI-82/83 graphing calculator. Various amounts of the carbonate are reacted with a constant amount of HCl.
Roser, Charles E.; McCluskey, Catherine L. J. Chem. Educ. 1999, 76, 638.
Stoichiometry |
Gases |
Laboratory Computing / Interfacing
|
Using CBL Technology and a Graphing Calculator To Teach the Kinetics of Consecutive First-Order Reactions José E. Cortés-Figueroa and Deborah A. Moore
This work proposes a demonstration to introduce first-order reactions using the CBL system. It then presents the analysis of two consecutive first-order reactions. The values of the rate constants that govern each reaction's rate are determined using the graphing and statistical capabilities of a TI-83 calculator.
Cortés-Figueroa, José E.; Moore, Deborah A. J. Chem. Educ. 1999, 76, 635.
Kinetics |
Laboratory Computing / Interfacing |
Rate Law
|
A Demonstration of Ideal Gas Principles Using a Football William D. Bare and Lester Andrews
A class demonstration and cooperative learning activity in which the ideal gas law is applied to determine the volume of a football is described. The mass of an air-filled football is recorded at two or more pressures, and students are asked to use these data to solve problems involving the volume, pressure, and mass of the football and the molecular weight of the gas in the ball.
Bare, William D.; Andrews, Lester. J. Chem. Educ. 1999, 76, 622.
Gases |
Applications of Chemistry
|
Alka Seltzer Poppers: An Interactive Exploration A. M. Sarquis and L. M. Woodward
This experiment illustrates concepts concerning the pressure-volume relationship of gases, solubility relationships of both gases and solids in liquids relative to temperature, the kinetics of the reaction of Alka Seltzer in water, and acid-base chemistry.
Sarquis, Arlyne M.; Woodward, L. M. J. Chem. Educ. 1999, 76, 385.
Acids / Bases |
Gases |
Kinetics |
Aqueous Solution Chemistry
|
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
|
The Fizz Keeper, a Case Study in Chemical Education, Equilibrium, and Kinetics Reed Howald
The chemistry of the loss of carbonation from carbonated beverages on storage is considered. Increasing the pressure of CO2(g) will restore carbonation, but an increase in pressure adding air should not affect the equilibria. It can and does, however, affect the kinetics-the rate at which a new equilibrium is established. Thus the Fizz Keeper is effective for storage of resealed pop containers for hours, but not for periods of weeks or months.
Howald, Reed. J. Chem. Educ. 1999, 76, 208.
Transport Properties |
Equilibrium |
Gases |
Kinetics |
Aqueous Solution Chemistry |
Consumer Chemistry |
Applications of Chemistry
|
A Precise Method for Determining the CO2 Content of Carbonate Materials Donald L. Pile, Alana S. Benjamin, Klaus S. Lackner, Christopher H. Wendt, and Darryl P. Butt
The design and use of a buret apparatus for CO2 gas capture and mass determination are described. The derivation of a comprehensive equation to determine the CO2 mass and percent carbonation of the material is outlined. Experimental factors such as temperature and pressure, including elevation effects, and apparatus parameters are discussed and incorporated into one general equation.
Pile, Donald L.; Benjamin, Alana S.; Lackner, Klaus S.; Wendt, Christopher H.; Butt, Darryl P. J. Chem. Educ. 1998, 75, 1610.
Laboratory Equipment / Apparatus |
Gases |
Quantitative Analysis
|
Gas Experiments with Plastic Soda Bottles Patrick Kavanah and Arden P. Zipp
The construction and use of a new device to study gases is described. The device, which is made from a plastic soda bottle and an automobile tire valve, can be used to demonstrate that air has mass, find the mass of the "evacuated" device, determine the molar mass of air and other gases, investigate the pressure-volume relationship, and build a cloud chamber.
Kavanah, Patrick; Zipp, Arden P. J. Chem. Educ. 1998, 75, 1405.
Gases |
Laboratory Equipment / Apparatus
|
The Best of Chem 13 News Kathy Thorsen
A variety of suggestions for instructional activities in introductory chemistry from Chem 13 News.
Thorsen, Kathy. J. Chem. Educ. 1998, 75, 1368.
Microscale Lab |
Gases |
Stoichiometry
|
Ernest Rutherford, Avogadro's Number, and Chemical Kinetics I. A. Leenson
The paper presents a way for students to use data from Rutherford's works (1908 - 1911) in order to determine one of the most precise values of Avogadro Constant available at the beginning of the century.
Leenson, I. A. J. Chem. Educ. 1998, 75, 998.
Learning Theories |
Nuclear / Radiochemistry |
Kinetics
|
Experimentally Determining the Molar Mass of Carbon Dioxide Using a Mylar Balloon Barbara Albers Jackson and David J. Crouse
The molar mass of carbon dioxide was experimentally determined using a Mylar balloon. Mylar balloons are lightweight, have a fixed definite volume, and require minimal additional pressure for inflation. Using the Ideal Gas Equation, the number of moles of air in the balloon was calculated.
Jackson, Barbara Albers; Crouse, David J. J. Chem. Educ. 1998, 75, 997.
Gases |
Physical Properties
|
Thermal Physics (and Some Chemistry) of the Atmosphere Stephen K. Lower
An exploration of how the temperature of the atmosphere varies with altitude can serve as a useful means of illustrating some important principles relating to the behavior of gases and to the absorption and transformation of radiant energy.
Lower, Stephen K. J. Chem. Educ. 1998, 75, 837.
Atmospheric Chemistry |
Gases
|
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
|
Small-Scale Kinetic Study of the Catalyzed Decomposition of Hydrogen Peroxide Ronald O. Ragsdale, Jan C. Vanderhooft , and Arden P. Zipp
The decomposition of hydrogen peroxide can be studied directly and quickly by determining the rate of formation of oxygen bubbles produced. This experiment, like the iodine clock reaction, provides quantitative measurements for a general chemistry course.
Ragsdale, Ronald O.; Vanderhooft , Jan C.; Zipp, Arden P. J. Chem. Educ. 1998, 75, 215.
Catalysis |
Kinetics |
Microscale Lab
|
A Simplified Determination of Percent Oxygen in Air Chin-Hsiang Fang
A simple, safe, and rapid experiment for determining the percent of oxygen in air is given.
Fang, Chin-Hsiang. J. Chem. Educ. 1998, 75, 58.
Gases |
Qualitative Analysis |
Quantitative Analysis |
Quantitative Analysis
|
On Laboratory Work Dave Olney
Suggestions for maximizing learning in the laboratory.
Olney, Dave. J. Chem. Educ. 1997, 74, 1343.
Gases |
Laboratory Computing / Interfacing |
Microscale Lab
|
Formation and Dimerization of NO2 A General Chemistry Experiment April D. Hennis, C. Scott Highberger, and Serge Schreiner*
A general chemistry experiment which illustrates Gay-Lussac's law of combining volumes. Students are able to determine the partial pressures and equilibrium constant for the formation and dimerization of NO2. The experiment readily provides students with data that can be manipulated with a common spreadsheet.
Hennis, April D.; Highberger, C. Scott; Schreiner, Serge. J. Chem. Educ. 1997, 74, 1340.
Gases |
Equilibrium |
Quantitative Analysis |
Stoichiometry
|
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
|
The Coupling of Related Demonstrations to Illustrate Principles in Chemical Kinetics and Equilibrium Richard A. Pacer
Two very simple lecture demonstrations, both involving the reaction of magnesium with one or more dilute acids, are linked together to illustrate principles in chemical kinetics and equilibrium.
Pacer, Richard A. J. Chem. Educ. 1997, 74, 543.
Learning Theories |
Acids / Bases |
Equilibrium |
Kinetics |
Rate Law |
Reactions
|
A U-Tube Experiment To Discover the Curve in Boyle's Law Thomas G. Richmond and Amy Parr
A discovery-style experiment is described to enable introductory chemistry students to determine the pressure versus volume behavior of a gas over a wide pressure range to "discover" Boyle's Law.
Richmond, Thomas G.; Parr, Amy. J. Chem. Educ. 1997, 74, 414.
Gases |
Laboratory Equipment / Apparatus
|
A Simple Boyle's Law Experiment Don L. Lewis
Student-conducted experiments over a range of pressures from about 14 psi to about 120 psi can safely and accurately be made utilizing a 60 ml syringe and an ordinary bathroom scale. No pressure gauge is required and no value for initial pressure in the syringe (near atmospheric pressure) need be assumed.
Lewis, Don L. J. Chem. Educ. 1997, 74, 209.
Gases
|
Egg in the Bottle (2) Moran, Michael
The cause of the pressure drop in the bottle is due to the cooling of high-temperature gases.
Moran, Michael J. Chem. Educ. 1996, 73, A189.
Gases
|
Egg in the Bottle (1) DeLorenzo, Ronald
The cooling of gas and the condensation of water vapor must be considered in addition to the loss of oxygen in reducing the pressure inside the glass bottle.
DeLorenzo, Ronald J. Chem. Educ. 1996, 73, A188.
Gases
|
Notes on Vapor Pressure Equilibria Measurements Albert G. Krieger, John W. Henderson
Freshman students at our institution use manometers and 24/40 ground-glass distillation apparatus (abandoned by our organic chemistry classes) to measure boiling points at reduced pressures. We have found that the availability of state-of-the-art equipment need not limit the ability to teach and demonstrate fundamental principles
Krieger, Albert G.; Henderson, John W. J. Chem. Educ. 1996, 73, 1039.
Gases |
Physical Properties
|
Small-Scale Experiments Involving Gas Evolution Brouwer, H.
Apparatus for measuring very small volume changes of gases and several experimental procedures involving the evolution of gases.
Brouwer, H. J. Chem. Educ. 1995, 72, A100.
Gases |
Laboratory Equipment / Apparatus |
Stoichiometry |
Acids / Bases |
Reactions |
Mechanisms of Reactions |
Microscale Lab
|
A Simple and Convenient Microscale Procedure for Investigation of Charles' Law Snyder, Donald M.
Experimental procedure for establishing temperature/volume relationship for a gas and determining the value of absolute zero using very simple equipment; includes sample data and analysis.
Snyder, Donald M. J. Chem. Educ. 1995, 72, A98.
Gases |
Calorimetry / Thermochemistry |
Microscale Lab
|
Dynamite Demo? Dale D. Clyde
Caution for boiling-water-with-ice demonstration.
Clyde, Dale D. J. Chem. Educ. 1995, 72, 1130.
Phases / Phase Transitions / Diagrams |
Liquids |
Gases
|
Entertaining Chemistry John F. Elsworth
"A Volcanic Serpent" (ammonium dichromate), "A Homemade Hydrogen Rocket", and "Johnny's Saga in Chemistry" (sulfuric acid + calcium carbonate) demonstrations.
Elsworth, John F. J. Chem. Educ. 1995, 72, 1128.
Reactions |
Acids / Bases |
Gases
|
The Environmental Chemistry of Trace Atmospheric Gases William C. Trogler
Information regarding the composition of trace gases in the Earth's atmosphere, changes in these amounts, their sources, and potential future impact on the environment.
Trogler, William C. J. Chem. Educ. 1995, 72, 973.
Gases |
Atmospheric Chemistry
|
A Systematic Experimental Test of the Ideal Gas Equation for the General Chemistry Laboratory Luis H. Blanco and Carmen M. Romero
A series of experiments that study all the gas laws in an integrated fashion.
Blanco, Luis H.; Romero, Carmen M. J. Chem. Educ. 1995, 72, 933.
Gases |
Kinetic-Molecular Theory
|
Ammonia Fountain and Density Gradient Column Miroslav Proksa
Demonstration combining the ammonia fountain with an acid-base indicator density column.
Proksa, Miroslav. J. Chem. Educ. 1995, 72, 931.
Solutions / Solvents |
Aqueous Solution Chemistry |
Physical Properties |
Gases |
Acids / Bases
|
Multiple Burning Heaps of Color-- An Elegant Variation of a Flame Test Eugene T. Smith
Making the ammonia fountain demonstration faster and more reliable using a common syringe.
Smith, Eugene T. J. Chem. Educ. 1995, 72, 828.
Laboratory Equipment / Apparatus |
Gases |
Solutions / Solvents |
Amines / Ammonium Compounds
|
More Chemistry in a Soda Bottle: A Conservation of Mass Activity Daniel Q. Duffy, Stephanie A. Shaw, William O. Bare, and Kenneth A. Goldsby
Conservation of mass activity using vinegar and baking soda in a 2-L soda bottle.
Duffy, Daniel Q.; Shaw, Stephanie A.; Bare, William D.; Goldsby, Kenneth A. J. Chem. Educ. 1995, 72, 734.
Reactions |
Gases |
Acids / Bases
|
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
|
A Transferable Gas Container (TGC): Improving the Balloon Inert Atmosphere Technique Bohac, Andrej
Apparatus for transferring inert gases using toy balloon and rubber tubing.
Bohac, Andrej J. Chem. Educ. 1995, 72, 263.
Laboratory Equipment / Apparatus |
Gases
|
Experiments for Modern Introductory Chemistry: The Temperature Dependence of Vapor Pressure Kildahl, Nicholas; Berka, Ladislav H.
Gas chromatography experiment that allows the discovery of the temperature dependence of the vapor pressure of a pure liquid; includes sample data and analysis.
Kildahl, Nicholas; Berka, Ladislav H. J. Chem. Educ. 1995, 72, 258.
Gases |
Liquids |
Gas Chromatography
|
Charles' Law of Gases: A Simple Experimental Demonstration Petty, John T.
Experimental procedure for demonstrating Charles' law.
Petty, John T. J. Chem. Educ. 1995, 72, 257.
Gases
|
Raoult's Law Is a Deception Hawkes, Stephen J.
Argument that Raoult's law should be omitted from introductory chemistry courses because of limited applicability and usefulness at that level of study.
Hawkes, Stephen J. J. Chem. Educ. 1995, 72, 204.
Rate Law |
Aqueous Solution Chemistry
|
A Charles' Law Experiment for Beginning Students Rockley, Mark G.; Rockley, Natalie L.
Experimental procedure and simple apparatus for illustrating Charles' Law and determining absolute zero; sample data and analysis are included.
Rockley, Mark G.; Rockley, Natalie L. J. Chem. Educ. 1995, 72, 179.
Gases |
Laboratory Equipment / Apparatus
|
Journey around a Phase Diagram Kildahl, Nicholas K.
This paper deals in depth with questions that arise from phase diagrams in an introductory level chemistry course.
Kildahl, Nicholas K. J. Chem. Educ. 1994, 71, 1052.
Phases / Phase Transitions / Diagrams |
Gases |
Liquids
|
Soda Water, Supercooling or Freezing Point Depression? Brooker, Murray H.
Composition, preparation, properties, and behavior of soda water.
Brooker, Murray H. J. Chem. Educ. 1994, 71, 903.
Gases |
Water / Water Chemistry |
Precipitation / Solubility |
Solutions / Solvents |
Consumer Chemistry
|
A New Quantitative Pressure-Volume Experiment Based on the "Cartesian Diver" Thompson, Judith U. S.; Goldsby, Kenneth A.
Modified Cartesian Diver to illustrate qualitatively and quantitatively the inverse, nonlinear relationship between gas pressure and volume.
Thompson, Judith U. S.; Goldsby, Kenneth A. J. Chem. Educ. 1994, 71, 801.
Gases
|
Dynamic Computer Simulation of the Motion of Gas Molecules Turner, Dean E.
165. Bits and pieces, 52. A program that simulates the motion of gas particles and illustrates the effects of temperature, mass, and volume.
Turner, Dean E. J. Chem. Educ. 1994, 71, 784.
Kinetic-Molecular Theory |
Gases
|
Experiments for Modern Introductory Chemistry: Intermolecular Forces and Raoult's Law Berka, Ladislav H.; Kildahl, Nicholas
Procedure that illustrates the liquid-vapor phase equilibrium of ideal and nonideal solutions.
Berka, Ladislav H.; Kildahl, Nicholas J. Chem. Educ. 1994, 71, 613.
Noncovalent Interactions |
Gas Chromatography |
Gases |
Liquids |
Equilibrium |
Solutions / Solvents
|
Demonstrating Simultaneous Boiling and Freezing (2) Ellison, Mike
Simple method of demonstrating simultaneous boiling and freezing of water using reduced pressure.
Ellison, Mike J. Chem. Educ. 1994, 71, 536.
Gases |
Physical Properties
|
Demonstrating Simultaneous Boiling and Freezing (1) Hiza, Mark R.
Simple method of demonstrating simultaneous boiling and freezing of water using reduced pressure.
Hiza, Mark R. J. Chem. Educ. 1994, 71, 536.
Gases |
Physical Properties
|
Solubility of CO2: A Variation of the Experiment Measuring Standard Molar Volume of a Gas Koster, David F.; Trimble, Russell F.
Carbon dioxide is formed in a molar volume experiment and the difference between the expected and actual volume of the gas is used to determine its solubility.
Koster, David F.; Trimble, Russell F. J. Chem. Educ. 1994, 71, 528.
Gases |
Precipitation / Solubility
|
Collapsing Containers Brown, Justina L.; Battino, Rubin
Using plastic containers instead of metal containers in air pressure demonstrations.
Brown, Justina L.; Battino, Rubin J. Chem. Educ. 1994, 71, 514.
Gases |
Physical Properties
|
Computer-interfaced apparatus to study osmosis and diffusion Fox, John N.; Hershman, Kenneth; Peard, Terry
Two experiments that lend themselves particularly well to computer interfacing dealing with osmosis and gas diffusion.
Fox, John N.; Hershman, Kenneth; Peard, Terry J. Chem. Educ. 1993, 70, A258.
Gases |
Laboratory Computing / Interfacing
|
Pictorial analogies IX: Liquids and their properties Fortman, John J.
Liquids on the molecular level, surface tension, and vapor pressure are explained through visual analogies of a class reunion and movie patrons.
Fortman, John J. J. Chem. Educ. 1993, 70, 881.
Liquids |
Gases |
Surface Science
|
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
|
Proper glove box etiquette Senn, Peter.
Additional considerations for an activity that appeared in this Journal in June, 1991 page 508.
Senn, Peter. J. Chem. Educ. 1993, 70, 519.
Gases
|
To bubble or not to bubble: Demonstrating Boyle's law Hughes, Elvin, Jr.; Holmes, L. H., Jr.
A simple demonstration to introduce pressure.
Hughes, Elvin, Jr.; Holmes, L. H., Jr. J. Chem. Educ. 1993, 70, 492.
Gases
|
An efficient and inexpensive device for measurement of gas volume Lieu, Van T.
Diagram and description of a device for measuring gas volume that yields good results.
Lieu, Van T. J. Chem. Educ. 1993, 70, 420.
Gases |
Laboratory Equipment / Apparatus
|
How vacuum cleaners pick up paper: Demonstrating the relationship between air pressure and vacuums Neils, Thomas L.
A demonstration to introduce the study of air pressure in general chemistry.
Neils, Thomas L. J. Chem. Educ. 1993, 70, 327.
Gases
|
Revealing the secret of the Arctic bomb Pearson, Earl F.
Arctic bombs and hurricanes can appear to be contradictory to gas law concepts commonly taught to chemistry students. While these phenomena can be explained as applications of simple gas laws, the explanations can be more effective if an apparent contradiction is drawn between students' understanding and the observed pressure-temperature relationship in these two examples.
Pearson, Earl F. J. Chem. Educ. 1993, 70, 315.
Gases |
Enrichment / Review Materials
|
LIMSport (II): Use of the Interfaced Balance for Pressure Measurements, Streamlined Syntheses, and Titrations Vitz, Ed
145. LIMSport facilitates direct acquisition of data from a variety of sensors into a spreadsheet.. This article explores the use of LIMSport in understanding gas laws.
Vitz, Ed J. Chem. Educ. 1993, 70, 63.
Gases |
Instrumental Methods
|
Gas reactions in plastic bags: Relating laboratory observations to the atomic-molecular model Robinson, Maurice; Barrow, Gordon M.
Carrying out chemical reactions in Ziplock bags to investigate a variety of chemical concepts.
Robinson, Maurice; Barrow, Gordon M. J. Chem. Educ. 1992, 69, 1026.
Kinetic-Molecular Theory |
Gases |
Reactions |
Acids / Bases |
Oxidation / Reduction |
Photochemistry |
Atmospheric Chemistry |
Physical Properties
|
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
|
Simple and inexpensive kinetics: A student laboratory experiment and demonstration Erwin, David K.
Laboratory experimentation, as well as in-class demonstration, involving the study of chemical kinetics can be performed using this safe, simple, and inexpensive apparatus. This apparatus requires only that systems to be studied must produce a gaseous product that can displace water.
Erwin, David K. J. Chem. Educ. 1992, 69, 926.
Kinetics |
Qualitative Analysis |
Quantitative Analysis |
Rate Law |
Laboratory Equipment / Apparatus
|
Equipment for gas law experiments Hennings, David G.
Using the plastic bottles sold with popcorn as leveling bulbs.
Hennings, David G. J. Chem. Educ. 1992, 69, 773.
Gases |
Laboratory Equipment / Apparatus
|
Hot and cold running methane Stamm, Daniel M.
A series of interesting demonstrations involving liquid nitrogen.
Stamm, Daniel M. J. Chem. Educ. 1992, 69, 762.
Gases
|
A modern vapor pressure apparatus based on the isoteniscope. Van Hecke, Gerald R.
Equipment used for vapor pressure measurements that eliminates use of a mercury manometer.
Van Hecke, Gerald R. J. Chem. Educ. 1992, 69, 681.
Laboratory Equipment / Apparatus |
Gases |
Liquids
|
Three methods for studying the kinetics of the halogenation of acetone. Birk, James P.; Walters, David L.
Three methods for carrying out a kinetic study of the reaction between propanone and elemental iodine.
Birk, James P.; Walters, David L. J. Chem. Educ. 1992, 69, 585.
Aldehydes / Ketones |
Kinetics |
Spectroscopy |
Rate Law
|
Fast molecular motion Knox, Kerro
A demonstration that shows that molecules do indeed move very fast and over long distances in a short time when nothing is in the way.
Knox, Kerro J. Chem. Educ. 1992, 69, 574.
Gases |
Kinetic-Molecular Theory
|
Simple soda bottle solubility and equilibria Snyder, Cheryl A.; Snyder, Dudley C.
Using a bottle of selzter water and bromocresol green to demonstrate gas-liquid solubility (carbon dioxide in water).
Snyder, Cheryl A.; Snyder, Dudley C. J. Chem. Educ. 1992, 69, 573.
Solutions / Solvents |
Precipitation / Solubility |
Equilibrium |
Gases |
Liquids |
Aqueous Solution Chemistry |
Water / Water Chemistry
|
The kinetic molecular theory and the weighing of gas samples Brenner, Henry C.
How is it possible to weigh gas samples since the molecules are constantly moving around and not always in contact with the floor of the container?
Brenner, Henry C. J. Chem. Educ. 1992, 69, 558.
Kinetic-Molecular Theory |
Gases |
Physical Properties
|
Pressure determinations using open-end manometers. Desmarais, George.
Method to increase students' understanding of and ability to quantify the level changes in a mercury manometer.
Desmarais, George. J. Chem. Educ. 1992, 69, 498.
Gases
|
A simple generator for common gases at atmospheric pressure Elsworth, John F.
The current high cost of either a Kipps generator for producing hydrogen sulfide in the undergraduate laboratory, or of the bottled gas, led the writer to construct a simple, economical and efficient generator for use in a laboratory fitted with an efficient fume hood.
Elsworth, John F. J. Chem. Educ. 1992, 69, 419.
Gases |
Laboratory Equipment / Apparatus
|
Vapor pressure demonstrations using a butane lighter Delumyea, R. Del
The concept of the change of state of matter and particularly the volatitlity of liquids is an important concept taught in introductory chemistry courses.
Delumyea, R. Del J. Chem. Educ. 1992, 69, 321.
Gases |
Physical Properties |
Liquids |
Phases / Phase Transitions / Diagrams
|
An "egg-splosive" demonstration. Becker, Robert.
The following demonstration uses an egg to demonstrate the explosive power of a combustible gaseous mixture.
Becker, Robert. J. Chem. Educ. 1992, 69, 229.
Gases
|
Does a one-molecule gas obey Boyle's law? Rhodes, Gail
Because the kinetic molecular theory provides a plausible explanation for the lawful behavior of gases, it should be treated in enough depth to show students that the theory accounts for all of the important aspects of ideal gas behavior.
Rhodes, Gail J. Chem. Educ. 1992, 69, 16.
Gases |
Kinetic-Molecular Theory
|
Inexpensive gas law apparatus Garrett, D. D.; Banta, M. C.; Arney, B. E.
The apparatus described in this paper avoids the problems associated with mercury as well as eliminating the friction problems usually encountered with the disposable syringes having rubber plunger tips.
Garrett, D. D.; Banta, M. C.; Arney, B. E. J. Chem. Educ. 1991, 68, 667.
Gases |
Laboratory Equipment / Apparatus
|
Soap bubble respirometry Cummins, Ken
Using the soap bubble respirometer to measure the vapor pressure of hexane over a temperature range.
Cummins, Ken J. Chem. Educ. 1991, 68, 617.
Gases |
Kinetic-Molecular Theory
|
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
|
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
|
Overhead projection of Graham's law of gaseous diffusion Epp, Dianne N.
Demonstration of gaseous diffusion through the combination of NH3 and HCl to produce NH4Cl.
Epp, Dianne N. J. Chem. Educ. 1990, 67, 1061.
Gases |
Transport Properties
|
Reduction of permanganate: A kinetics demonstration for general chemistry Steffel, Margaret J.
Using the reduction of MnO4- to Mn2+ in aqueous solution to demonstrate the four factors that control reaction rates in solution: the natures of the reactants, concentrations of the reactants, temperature, and the presence of a catalyst.
Steffel, Margaret J. J. Chem. Educ. 1990, 67, 598.
Kinetics |
Rate Law |
Catalysis |
Oxidation / Reduction
|
A visual demonstration of Raoult's law Wilson, Archie S.
Reducing the vapor pressure of bromine by adding chloroform.
Wilson, Archie S. J. Chem. Educ. 1990, 67, 598.
Gases |
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
|
Improvements to demonstration of vapor pressure (author response) Richardson, W. S.
The incorporation of a calculation using the ideal gas law as suggested by Hambly is a welcomed improvement.
Richardson, W. S. J. Chem. Educ. 1990, 67, 278.
Gases
|
Improvements to demonstration of vapor pressure Hambly, Gordon F.
The author is offering some improvements to a recent publication on the "Demonstration of Vapor Pressure."
Hambly, Gordon F. J. Chem. Educ. 1990, 67, 278.
Gases
|
Concept learning versus problem solving: Revisited Sawrey, Barbara A.
A student's ability to solve a numerical problem does not guarantee conceptual understanding of the molecular basis of the problem.
Sawrey, Barbara A. J. Chem. Educ. 1990, 67, 253.
Learning Theories |
Stoichiometry |
Gases
|
A simple apparatus to demonstrate differing gas diffusion rates (Graham's law) Keller, Philip C.
The apparatus described in this note dramatically demonstrates relative diffusion rate effects for common gases like methane and carbon dioxide.
Keller, Philip C. J. Chem. Educ. 1990, 67, 160.
Gases |
Laboratory Equipment / Apparatus |
Separation Science
|
A precise determination of absolute zero Strange, Ronald S.; Lang, Frank T.
Excellent extrapolations to absolute zero can be obtained for dry air using a simple apparatus constructed from an Erlenmeyer flask, an oil manostat and a plastic syringe.
Strange, Ronald S.; Lang, Frank T. J. Chem. Educ. 1989, 66, 1054.
Gases |
Laboratory Equipment / Apparatus
|
The ideal gas law at the center of the sun Clark, David B.
Applying the ideal gas law to conditions found at the center of the sun.
Clark, David B. J. Chem. Educ. 1989, 66, 826.
Gases |
Astrochemistry
|
A microscale study of gaseous diffusion Epp, Dianne N.; Lyons, Edward J.; Brooks, David W.
The following microscale experiment compares qualitatively the rates of diffusion in air of chlorine molecules and ammonia molecules.
Epp, Dianne N.; Lyons, Edward J.; Brooks, David W. J. Chem. Educ. 1989, 66, 436.
Gases |
Microscale Lab
|
Preparation and cleaning of low-cost plastic manometers Pollnow, Gilbert F.
The author has developed an improved unbreakable manometer.
Pollnow, Gilbert F. J. Chem. Educ. 1989, 66, 333.
Gases |
Laboratory Equipment / Apparatus
|
Determination of the universal gas constant Lebman, Thomas A.; Harms, Gwen
An experiment for the calculation of R using R-PV/nT.
Lebman, Thomas A.; Harms, Gwen J. Chem. Educ. 1988, 65, 811.
Gases |
Stoichiometry
|
Some analogies for teaching rates/equilibrium Olney, David J.
This article presents several analogies for teaching rates and equilibrium developed by the author over his many years in the chemistry classroom that seem to be effective.
Olney, David J. J. Chem. Educ. 1988, 65, 696.
Kinetics |
Equilibrium
|
Soap bubbles and precipitate membranes: Two historical semipermeability experiments adapted for teaching purposes Nicolini, Nicoletta; Pentella, Antonio
These demonstrations are based on the historical experiments that established our understanding of semipermeability and osmosis.
Nicolini, Nicoletta; Pentella, Antonio J. Chem. Educ. 1988, 65, 614.
Gases |
Surface Science |
Transport Properties |
Electrochemistry
|
Will that pop bottle really go pop? An equilibrium question Deamer, David W.; Selinger, Benjamin K.
These authors challenge a claim that appeared in the journal *New Scientist* regarding carbon dioxide in carbonated beverages and equilibrium.
Deamer, David W.; Selinger, Benjamin K. J. Chem. Educ. 1988, 65, 518.
Applications of Chemistry |
Gases |
Equilibrium
|
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
|
A "stationery" kinetics experiment Hall, L.; Goherdhansingh, A.
The simple redox reaction that occurs between potassium permanganate and oxalic acid can be used to prepare an interesting disappearing ink that is the basis for a kinetics experiment for an introductory chemistry class.
Hall, L.; Goherdhansingh, A. J. Chem. Educ. 1988, 65, 142.
Kinetics
|
A metal bar to demonstrate one atmosphere Meloan, Clifton E.
This demonstration helps students gain a more intuitive understanding of units of pressure.
Meloan, Clifton E. J. Chem. Educ. 1988, 65, 69.
Gases |
Physical Properties
|
Chem Lab Simulations 1: Titrations and Chem Lab Simulations 2: Ideal Gas Law (Gelder, John) Zemke, Warren T.
Computer programs intended to serve as introductions for students before actual experimentation in the laboratory.
Zemke, Warren T. J. Chem. Educ. 1987, 64, A57.
Titration / Volumetric Analysis |
Gases |
Enrichment / Review Materials
|
Two fundamental constants McNaught, Ian J.; Peckham, Gavin D.
Experiment to produce accurate values for both the absolute zero of temperature and the gas constant.
McNaught, Ian J.; Peckham, Gavin D. J. Chem. Educ. 1987, 64, 999.
Gases
|
A Charles's Law/vapor pressure apparatus Hall, Philip K.
A simple apparatus to illustrate either Charles's law gas expansion of the vapor pressure created by liquids.
Hall, Philip K. J. Chem. Educ. 1987, 64, 969.
Gases |
Liquids
|
Demonstration of vapor pressure Richardson, W. S.
Demonstrating the vapor pressure of several different materials using a water manometer.
Richardson, W. S. J. Chem. Educ. 1987, 64, 968.
Gases |
Phases / Phase Transitions / Diagrams |
Liquids
|
Physical and chemical properties Boschmann, Erwin
A series of overhead demonstrations regarding physical and chemical properties.
Boschmann, Erwin J. Chem. Educ. 1987, 64, 891.
Physical Properties |
Liquids |
Precipitation / Solubility |
Magnetic Properties |
Kinetic-Molecular Theory |
Crystals / Crystallography |
Gases
|
Charles's law: Students develop their own procedure Rose, Diane
Students are asked to write their own procedure and execute it in the lab.
Rose, Diane J. Chem. Educ. 1987, 64, 712.
Gases
|
An indicating rupture disk for gas cylinders Bruno, Thomas J.
A device to allow a determination of the approximate condition of the rupture disk in compressed gas cylinders.
Bruno, Thomas J. J. Chem. Educ. 1987, 64, 557.
Gases |
Laboratory Management
|
An example of a constant rate reaction Tawarab, Khalid M.
A simple experiment whose rate of reaction (a burning candle) proceeds at constant conditions.
Tawarab, Khalid M. J. Chem. Educ. 1987, 64, 534.
Rate Law |
Kinetics
|
Control of variables and the conservation of matter Giachino, Gary G.
Demonstrates the conservation of matter, but its main value lies in its illustration of the need to control variables and the difficulty this may entail - particularly if a variable is "hidden"; uses a burning candle in a glass flask.
Giachino, Gary G. J. Chem. Educ. 1987, 64, 353.
Gases
|
Coupled oscillations Onwood, D. P.
Demonstrating coupled oscillations using pendulums.
Onwood, D. P. J. Chem. Educ. 1987, 64, 351.
Kinetics
|
A safe cell for viewing the critical point of CO2 Botch, Beatrice; Battino, Rubin
Design, construction, and use of a safe cell for viewing the critical point of CO2.
Botch, Beatrice; Battino, Rubin J. Chem. Educ. 1987, 64, 347.
Laboratory Equipment / Apparatus |
Phases / Phase Transitions / Diagrams |
Gases |
Liquids
|
Simple determination of Henry's law constant for carbon dioxide Levy, Jack B.; Hornack, Fred M.; Levy, Matthew A.
With the aid of inexpensive pressure gauges available from automotive supply stores, the solubility of carbon dioxide in carbonated beverages or other solutions can be studied.
Levy, Jack B.; Hornack, Fred M.; Levy, Matthew A. J. Chem. Educ. 1987, 64, 260.
Gases |
Solutions / Solvents
|
Annotating reaction equations Tykodi, R. J.
Annotating aqueous solution reactions fosters recognition of the fundamental reaction categories; ready recognition of a reaction type is the first step toward understanding the "whys and wherefores" inherent in the reaction.
Tykodi, R. J. J. Chem. Educ. 1987, 64, 243.
Aqueous Solution Chemistry |
Reactions |
Acids / Bases |
Gases |
Precipitation / Solubility |
Oxidation / Reduction
|
Carbon dioxide: Its principal properties displayed and discussed Bent, Henry A.
The principal properties of carbon dioxide demonstrated and discussed.
Bent, Henry A. J. Chem. Educ. 1987, 64, 167.
Physical Properties |
Phases / Phase Transitions / Diagrams |
Gases |
Kinetic-Molecular Theory
|
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
|
Gas cans and gas cubes: Visualizing Avogadro's Law Bouma, J.
The author shares a strategy for making gas laws "visible" for students.
Bouma, J. J. Chem. Educ. 1986, 63, 586.
Gases |
Stoichiometry
|
Chemical knowledge versus conventional "wisdom" Steffel, Margaret J.
A question about the physical properties of gases that rewards students with some knowledge of aviation.
Steffel, Margaret J. J. Chem. Educ. 1986, 63, 317.
Gases
|
TRS-80 Chemistry Lab, Volume 1, Review II (Hallgren, Richard C.) Beck, James D.
Programs covering the kinetic theory, Charles' law, Boyle' law, titration, and solubility.
Beck, James D. J. Chem. Educ. 1985, 62, A106.
Kinetic-Molecular Theory |
Gases |
Titration / Volumetric Analysis |
Precipitation / Solubility
|
TRS-80 Chemistry Lab, Volume 1, Review I (Hallgren, Richard C.) Rowe, Frederick J.
Programs covering the kinetic theory, Charles' law, Boyle' law, titration, and solubility.
Rowe, Frederick J. J. Chem. Educ. 1985, 62, A105.
Kinetic-Molecular Theory |
Gases |
Titration / Volumetric Analysis |
Precipitation / Solubility
|
Molecular size and Raoult's Law Kovac, Jeffrey
An additional cause for deviations from Raoult's Law that is rarely, if ever, mentioned in freshman chemistry texts.
Kovac, Jeffrey J. Chem. Educ. 1985, 62, 1090.
Molecular Properties / Structure |
Physical Properties |
Solutions / Solvents |
Gases
|
Le Châtelier's Principle Knox, Kerro
Question involving effect of increasing the pressure on the N2 + 3H2 <=> 2NH3 system.
Knox, Kerro J. Chem. Educ. 1985, 62, 863.
Equilibrium |
Gases
|
Measuring the atomic or molecular mass of a gas with a tire gauge and a butane lighter fluid can Bodner, George M.; Magginnis, Lenard J.
Also demonstrating the mass of air and the dependence of the pressure of a gas on the mass of the sample.
Bodner, George M.; Magginnis, Lenard J. J. Chem. Educ. 1985, 62, 434.
Atomic Properties / Structure |
Molecular Properties / Structure |
Alkanes / Cycloalkanes |
Gases
|
A comment on "The order of CH3CHO decomposition" Liu, Michael T. H.
The order of the decomposition of acetaldehyde is 3/2 or 1.5.
Liu, Michael T. H. J. Chem. Educ. 1985, 62, 399.
Aldehydes / Ketones |
Rate Law |
Kinetics
|
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
|
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
|
Cooking with chemistry Grosser, Arthur E.
Two demonstrations involving cooking eggs and suggestions for many more examples of cooking that illustrate important principles of chemistry. From the "State-of-the-Art Symposium for Chemical Educators: Chemistry of the Food Cycle".
Grosser, Arthur E. J. Chem. Educ. 1984, 61, 362.
Food Science |
Gases |
Acids / Bases |
Equilibrium |
Kinetics
|
Diffusion of gases - Kinetic molecular theory of gases Schlecht, K. D.
Changing the pressure inside a container with a porous surface through the diffusion of hydrogen or helium.
Schlecht, K. D. J. Chem. Educ. 1984, 61, 251.
Gases |
Transport Properties |
Kinetic-Molecular Theory
|
The density and apparent molecular weight of air Harris, Arlo D.
Simple procedure for determining the density and apparent molecular weight of air.
Harris, Arlo D. J. Chem. Educ. 1984, 61, 74.
Atmospheric Chemistry |
Gases |
Molecular Properties / Structure |
Physical Properties
|
Gas laws and gas behavior Schmuckler, Joseph S.
A collection of activities from past issues of the Journal and The Science Teacher.
Schmuckler, Joseph S. J. Chem. Educ. 1984, 61, 73.
Gases
|
Enduring distributions that deny Boltzmann Nash, Leonard K.
Examines two practical steady- state distributions: the atmosphere and its lapse rate and the ocean and its vertical quasi-uniformity.
Nash, Leonard K. J. Chem. Educ. 1984, 61, 22.
Atmospheric Chemistry |
Gases
|
Boyle's law experiment Hermens, Richard A.
This experiment regarding Boyle's law adheres to qualifications which allow the experiment to be meaningful to the students, is safe and simple to perform, low in cost, easy to set up and maintain, obtains reproducible results, and is capable of being performed in a reasonable length of time.
Hermens, Richard A. J. Chem. Educ. 1983, 60, 764.
Gases
|
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
|
Computer simulation of elementary chemical kinetics Nase, Martha L.; Seidman, Kurt
44. Bits and pieces, 16. The authors have developed several computer programs that simulate chemical kinetics for elementary first and second order processes. These programs can be used to generate kinetic data that can then be analyzed by the student in a variety of ways.
Nase, Martha L.; Seidman, Kurt J. Chem. Educ. 1983, 60, 734.
Kinetics |
Rate Law
|
NH4HC03: a stimulant for learning Richards, R. Ronald
Students, professors, and the literature have all been confused by the unusual dissociation equilibrium of NH4HCO3.
Richards, R. Ronald J. Chem. Educ. 1983, 60, 555.
Equilibrium |
Amines / Ammonium Compounds |
Gases
|
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
|
An effective demonstration of some properties of real vapors Metsger, D. Scott
The apparatus described in this article has been found by the authors to be the most effective in vividly illustrating the behavior of a nearly ideal gas to first year chemistry students.
Metsger, D. Scott J. Chem. Educ. 1983, 60, 67.
Laboratory Equipment / Apparatus |
Gases |
Physical Properties |
Solids
|
Boyle's law and the monster marshmallow Broniec, Rick
Evacuating the air surrounding a marshmallow with a vacuum pump.
Broniec, Rick J. Chem. Educ. 1982, 59, 974.
Gases
|
Vapor pressure apparatus for general chemistry Long, Joseph W.
A simple apparatus for collecting vapor pressure data; relies on a mercury manometer.
Long, Joseph W. J. Chem. Educ. 1982, 59, 933.
Laboratory Equipment / Apparatus |
Phases / Phase Transitions / Diagrams |
Gases
|
Collapsing can Sands, Richard D.
Demonstrates the solubility of ammonia gas in water.
Sands, Richard D. J. Chem. Educ. 1982, 59, 866.
Gases |
Phases / Phase Transitions / Diagrams |
Precipitation / Solubility |
Aqueous Solution Chemistry
|
Boyle's law - A different view Sharma, B. D.
For a fixed mass of gas at constant temperature the energy of the gas is fixed and independent of its pressure and volume.
Sharma, B. D. J. Chem. Educ. 1982, 59, 827.
Gases
|
The titration of air with nitric oxide: An application of Gay-Lussac's law of combining volumes in a general chemistry experiment Everett, Kenneth G.
Gay-Lussac's law of combining volumes is demonstrated through the reaction between NO and the oxygen in air.
Everett, Kenneth G. J. Chem. Educ. 1982, 59, 802.
Titration / Volumetric Analysis |
Atmospheric Chemistry |
Gases
|
The use of a filmstrip projector to present a critical point demonstration Nyquist, H. LeRoy
A demonstration to illustrate the concepts of critical temperature and critical pressure.
Nyquist, H. LeRoy J. Chem. Educ. 1982, 59, 522.
Gases |
Liquids
|
A simple experiment for determining vapor pressure and enthalpy of vaporization of water Levinson, Gerald S.
It is possible to determine the vapor pressure of water using only a tall beaker, a graduated cylinder, and a thermometer.
Levinson, Gerald S. J. Chem. Educ. 1982, 59, 337.
Water / Water Chemistry |
Gases |
Phases / Phase Transitions / Diagrams
|
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
|
Cinema, flirts, snakes, and gases Hartwig, Dcio R.; Filho, Romeu C. Rocha
Explaining the kinetic behavior of gases through several analogies.
Hartwig, Dcio R.; Filho, Romeu C. Rocha J. Chem. Educ. 1982, 59, 295.
Kinetic-Molecular Theory |
Gases
|
Notes from physics journals Smith, Douglas D.
Solution with an index of refraction that matches that of Pyrex glass and a reverse cartesion diver.
Smith, Douglas D. J. Chem. Educ. 1982, 59, 243.
Gases |
Solutions / Solvents
|
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
|
Balloons and the teaching of chemistry Dewhurst, F.; Dewhurst, F. R.
Balloons are a remarkably useful tool for the chemical educationalist. Balloons can not only provide cheap, safe, and easy-to-use alternatives to more complex and costly equipment, but also they can be used as effective teaching aids to demonstrate principles of structural chemistry.
Dewhurst, F.; Dewhurst, F. R. J. Chem. Educ. 1981, 58, 44.
Gases |
Laboratory Equipment / Apparatus
|
Gases and their behavior Schmuckler, Joseph S.
Schmuckler, Joseph S. J. Chem. Educ. 1980, 57, 885.
Gases
|
Chemical Kinetics: Reaction Rates Mickey, Charles D.
Reviews the chemistry behind factors that influence the rates of chemical reactions.
Mickey, Charles D. J. Chem. Educ. 1980, 57, 659.
Rate Law |
Kinetics |
Reactions |
Catalysis
|
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
|
Properly opening a beer can and Boyle's law DeLorenzo, Ron
Why tapping the side of a can or bottle can reduce spray when opening.
DeLorenzo, Ron J. Chem. Educ. 1980, 57, 601.
Gases
|
Bicarbonate in Alka-Seltzer: A general chemistry experiment Peck, Larry; Irgolic, Kurt; O'Connor, Rod
Determining the percentage bicarbonate ion by mass in Alka-Seltzer.
Peck, Larry; Irgolic, Kurt; O'Connor, Rod J. Chem. Educ. 1980, 57, 517.
Quantitative Analysis |
Gases |
Stoichiometry |
Acids / Bases
|
PV work demonstration (Corridor demonstration) Koubek, E.
A hallway demonstration regarding the work done in pulling out a piston on display.
Koubek, E. J. Chem. Educ. 1980, 57, 374.
Gases
|
A chemistry lesson at Three Mile Island Mammano, Nicholas J.
Teaching principles of general chemistry through references made to the nuclear incident at Three Mile Island.
Mammano, Nicholas J. J. Chem. Educ. 1980, 57, 286.
Equilibrium |
Gases |
Stoichiometry |
Nonmajor Courses |
Nuclear / Radiochemistry |
Applications of Chemistry
|
Pressure measuring devices and pressure calculations Schultz, Charles W.
A question requiring an understanding of the principle of operation of pressure gauges.
Schultz, Charles W. J. Chem. Educ. 1980, 57, 285.
Gases
|
The solution: "Derivation of the ideal gas law" Bosch, Warren L.; Crawford, Crayton M.; Gensler, Walter J.; Haim, Albert; Levine, Ira N.; Linde, Peter F.; Salzsieder, John C.; Silberszye, Waldemar; Viehland, Larry A.; Waser, Jurg
A response to the misinterpretations that appeared in the referenced article regarding the gas laws.
Bosch, Warren L.; Crawford, Crayton M.; Gensler, Walter J.; Haim, Albert; Levine, Ira N.; Linde, Peter F.; Salzsieder, John C.; Silberszye, Waldemar; Viehland, Larry A.; Waser, Jurg J. Chem. Educ. 1980, 57, 201.
Gases
|
Balloon balance thermometer: A lecture demonstration of Charles' Law Carney, G. D.; Kern, C. W.
The balloon-balance thermometer makes use of air as a thermometric fluid, a water bath as the thermometric vessel, and the readings of a triple beam balance as a thermometer scale.
Carney, G. D.; Kern, C. W. J. Chem. Educ. 1979, 56, 823.
Gases
|
The gases of life J. Chem. Educ. Staff
Considers the topics of diffusion, oxygen transport through the lungs, oxygen in arterial blood, and CO2 transfer.
J. Chem. Educ. Staff J. Chem. Educ. 1979, 56, 748.
Gases |
Transport Properties |
Equilibrium
|
Catalysis Kolb, Doris
Definitions for and history of catalysts, speeding up chemical reactions, enzymes, and industrial catalysis.
Kolb, Doris J. Chem. Educ. 1979, 56, 743.
Catalysis |
Rate Law |
Enzymes |
Industrial Chemistry
|
Lecture demonstration of vanishing meniscus in vapor liquid transition Duus, H. C.
Shows how the interface between vapor and liquid propane vanishes.
Duus, H. C. J. Chem. Educ. 1979, 56, 614.
Liquids |
Gases |
Phases / Phase Transitions / Diagrams
|
The problem: "Derivation of the ideal gas law" Vaitkunas, John J.
Outline for a lesson on gases, and suggestions for approaches to the ideal gas law.
Vaitkunas, John J. J. Chem. Educ. 1979, 56, 530.
Gases
|
The variation of vapor pressure with temperature Davenport, Derek A.; Srinivasan, Viswanathan
Comparing the pressure of three cans of lighter fluid at different temperatures.
Davenport, Derek A.; Srinivasan, Viswanathan J. Chem. Educ. 1979, 56, 474.
Gases |
Kinetic-Molecular Theory
|
The temperature dependence of the equilibrium constant Burness, James H.
This exam question tests a student's ability to derive the temperature dependence of an equilibrium constant not by qualitatively applying Le Chatelier's principle, but by understanding the relationship between the kinetics of the equation and the value of Keq.
Burness, James H. J. Chem. Educ. 1979, 56, 395.
Equilibrium |
Kinetics
|
Ga(U)Ge pressure and absolute pressure Davenport, Derek A.
Air is progressively removed from a test tube; the pressure inside is measured using a standard tire-pressure gauge that is found to read atmospheric pressure when the test tube is fully evacuated.
Davenport, Derek A. J. Chem. Educ. 1979, 56, 322.
Gases
|
Boyle's law Davenport, Derek A.
Increasing weights are placed on a sealed syringe, compressing the air inside, and increasing weights pull the plunger from a held syringe, expanding the air inside. In both cases, plots of "P" vs. V are recorded.
Davenport, Derek A. J. Chem. Educ. 1979, 56, 322.
Gases
|
An experiment oriented approach to teaching the kinetic molecular theory Wiseman, Frank L., Jr.
A series of experiments designed to illustrate the kinetic molecular theory and the differences between solids, liquids, and gases.
Wiseman, Frank L., Jr. J. Chem. Educ. 1979, 56, 233.
Kinetic-Molecular Theory |
Gases |
Solids |
Liquids |
Nonmajor Courses
|
Participatory lecture demonstrations Battino, Rubin
Examples of participatory lecture demonstrations in chromatography, chemical kinetics, balancing equations, the gas laws, the kinetic-molecular theory, Henry's law, electronic energy levels in atoms, translational, vibrational, and rotational energies of molecules, and organic chemistry.
Battino, Rubin J. Chem. Educ. 1979, 56, 39.
Chromatography |
Kinetic-Molecular Theory |
Kinetics |
Stoichiometry |
Gases |
Atomic Properties / Structure |
Molecular Properties / Structure
|
A discovery experiment. CO2 soap bubble dynamics Millikan, Roger C.
Students often make a choice of major based upon the view of a subject that they derive from the beginning course. Rare are the chemistry courses that provide the excitement and chance for discovery, while providing a basic understanding of chemistry. This article describes an experiment that does provide such an opportunity.
Millikan, Roger C. J. Chem. Educ. 1978, 55, 807.
Gases |
Physical Properties |
Surface Science
|
The Color blind traffic light Boulanger, Mathilda M.
A fascinating oscillating reaction.
Boulanger, Mathilda M. J. Chem. Educ. 1978, 55, 584.
Kinetics
|
An Exercise with Boyle's law Moeller, Michael B.
A procedure for doing a demonstration of Boyles' law.
Moeller, Michael B. J. Chem. Educ. 1978, 55, 584.
Gases
|
Bubble pressure and volume. A demonstration experiment Christian, Sherril D.; Enwall, Eric
An interesting phenomenon which illustrates several important principles, is the dependence of the size of a soap bubble on pressure. The subject is introduced to the class by the black box experiment presented in this article.
Christian, Sherril D.; Enwall, Eric J. Chem. Educ. 1978, 55, 536.
Gases |
Surface Science
|
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
|
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
|
General chemistry-pressure measurement Steffel, Margaret J.
This question allows students to demonstrate the understanding of the operation of barometers and vapor pressure at a freshman level.
Steffel, Margaret J. J. Chem. Educ. 1978, 55, 102.
Gases |
Quantitative Analysis |
Laboratory Equipment / Apparatus
|
Molar volumes: Microscopic insight from macroscopic data Davenport, Derek A.; Fosterling, Robert B.; Srinivasan, Viswanathan
The molar volumes of the alkali metal halides; molar volumes of binary hydrogen compounds; molar volumes of the first transition series; molar volumes of the lanthanoids and actinoids; molar volumes of the carbon family; molar volumes of isotopically related species; aquated ions and ions in aqueous solution.
Davenport, Derek A.; Fosterling, Robert B.; Srinivasan, Viswanathan J. Chem. Educ. 1978, 55, 93.
Inner Transition Elements |
Metals |
Periodicity / Periodic Table |
Stoichiometry |
Gases |
Transition Elements |
Aqueous Solution Chemistry |
Isotopes
|
Reaction rates for a homogeneously catalyzed reaction Nechamkin, Howard; Keller, Elhannan; Goodkin, Jerome
The reaction of KMnO4 with hydrogen in an acidic medium is an example of a homogeneously catalyzed reaction that can be performed by college freshmen.
Nechamkin, Howard; Keller, Elhannan; Goodkin, Jerome J. Chem. Educ. 1977, 54, 775.
Rate Law |
Kinetics |
Catalysis
|
Gasoline vapor: An invisible pollutant Stephens, Edgar R.
An apparatus and procedure to demonstrate the substantial contribution vaporized gasoline makes to hydrocarbon pollution.
Stephens, Edgar R. J. Chem. Educ. 1977, 54, 682.
Physical Properties |
Gases |
Atmospheric Chemistry
|
Ultraviolet absorption of ozone Driscoll, Jerry A.
A demonstration of the absorption of ultraviolet radiation by ozone.
Driscoll, Jerry A. J. Chem. Educ. 1977, 54, 675.
Gases |
Atmospheric Chemistry
|
Water dipping kinetics. A physical analog for chemical kinetics Birk, James P.; Gunter, S. Kay
Physical analogs of zero-, first, and second-order kinetics using the volume of water transferred by a dipper oriented in different directions with respect to a basin of water.
Birk, James P.; Gunter, S. Kay J. Chem. Educ. 1977, 54, 557.
Kinetics |
Equilibrium |
Rate Law
|
Questions [and] Answers Campbell, J. A.
309-314. Six questions involving practical applications of chemistry.
Campbell, J. A. J. Chem. Educ. 1977, 54, 437.
Enrichment / Review Materials |
Toxicology |
Alcohols |
Gases |
Natural Products
|
Ideal and non-ideal gases. An experiment with surprise value Chirpich, Thomas P.
Compares the behavior of an ideal gas (air) with a non-ideal gas (water vapor) as they are cooled from 100C to room temperature.
Chirpich, Thomas P. J. Chem. Educ. 1977, 54, 378.
Gases
|
Simplified Boyle's Law demonstration Miller, Daniel W.
Placing a sealed syringe in bell jar attached to a vacuum pump and reading the volume of air inside the syringe at various reduced pressures.
Miller, Daniel W. J. Chem. Educ. 1977, 54, 245.
Gases
|
Chemical oscillations as an undergraduate experiment Deb, B. M.
Hitherto unreported observations regarding the Briggs-Rauscher oscillating system.
Deb, B. M. J. Chem. Educ. 1977, 54, 236.
Reactions |
Kinetics
|
Le Chtelier's principle: A laboratory exercise Friedman, Frederica
Le Chtelier's principle can be demonstrated by showing that water can boil at temperatures below 100C due to reduced vapor pressure.
Friedman, Frederica J. Chem. Educ. 1977, 54, 236.
Equilibrium |
Phases / Phase Transitions / Diagrams |
Gases |
Water / Water Chemistry
|
The Old Nassau reaction Alyea, Hubert N.
A description of the chemistry and history of the Old Nassau reactions.
Alyea, Hubert N. J. Chem. Educ. 1977, 54, 167.
Kinetics |
Reactions
|
Lab safety: The case of the errant cylinder Ozaruk, N.
The anchoring of compressed gas cylinders to keep them from being knocked over, with the accompanying possibility of breaking off the valve, is an accepted safe practice. However, there has been some skepticism as to what would have happened if a cylinder valve was knocked off. The author shares a vivid description that appeared in the National Safety Council Chemical Section Newsletter. Also: a high school safety rules booklet; a hazardous materials safety booklet; and wall charts on Laboratory Techniques and Laboratory Safety.
Ozaruk, N. J. Chem. Educ. 1976, 53, 373.
Laboratory Equipment / Apparatus |
Laboratory Management |
Gases
|
A computer program for calculation of boiling points at sub- and super-atmospheric pressures Davis, Charles C.; Wright, C. David
An interactive program has been written in Fortran IV for the IBM 370/125 which will compute the boiling points of organic compounds at a range of pressures.
Davis, Charles C.; Wright, C. David J. Chem. Educ. 1976, 53, 355.
Laboratory Computing / Interfacing |
Phases / Phase Transitions / Diagrams |
Gases
|
A computer program for calculation of boiling points at sub- and super-atmospheric pressures Davis, Charles C.; Wright, C. David
An interactive program has been written in Fortran IV for the IBM 370/125 which will compute the boiling points of organic compounds at a range of pressures.
Davis, Charles C.; Wright, C. David J. Chem. Educ. 1976, 53, 355.
Laboratory Computing / Interfacing |
Phases / Phase Transitions / Diagrams |
Gases
|
Ideal gas laws. Experiments for general chemistry Deal, Walter J.
Several gas-law experiments designed to verify the relationship PV = constant at constant temperature and to calculate the gas constant R.
Deal, Walter J. J. Chem. Educ. 1975, 52, 405.
Gases
|
Questions [and] Answers Campbell, J. A.
188-192. Five biochemistry related questions and their answers.
Campbell, J. A. J. Chem. Educ. 1975, 52, 390.
Enrichment / Review Materials |
Nuclear / Radiochemistry |
Chromatography |
Gases |
Nutrition
|
Capillary flow. A versatile analog for chemical kinetics Davenport, Derek A.
A number of novel ways in which capillary flow can be used as a mechanical analog for chemical kinetics.
Davenport, Derek A. J. Chem. Educ. 1975, 52, 379.
Kinetics
|
Effective insect fogging - The origin of sea breezes - Hot air balloons Plumb, Robert C.
Three applications of the changes in pressure or volume of a gas when its temperature is changed.
Plumb, Robert C. J. Chem. Educ. 1975, 52, 104.
Gases |
Applications of Chemistry
|
A Dalton's law experiment for students in the health sciences Feigl, Dorothy M.
The number of students who take an introductory chemistry course in preparation for the health sciences is increasing. This note is an illustration of Dalton's law of partial pressures adapted to demonstrate the ability of the lungs to effect the removal of excess dioxide from the body.
Feigl, Dorothy M. J. Chem. Educ. 1974, 51, 273.
Gases |
Biophysical Chemistry
|
Lecture experiment: A quantitative illustration of LeChatelier's principle Nelson, D. L.; Ginns, E. I.; Richtol, H. H.; Reeves, R. R.
A short experiment involving the popular gaseous nitrogen dioxide system has been developed into a lecture demonstration which quantitatively illustrates the behavior of a homogeneous gas-phase equilibrium under conditions of varying temperature and pressure.
Nelson, D. L.; Ginns, E. I.; Richtol, H. H.; Reeves, R. R. J. Chem. Educ. 1973, 50, 721.
Equilibrium |
Gases
|
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 Charles' Law experiment using a balloon or a plastic bag Murdock, Howard D.; Hawthorne, Robert M., Jr.
A general chemistry experiment that demonstrates Charles' Law clearly, quickly, and relatively quantitatively.
Murdock, Howard D.; Hawthorne, Robert M., Jr. J. Chem. Educ. 1973, 50, 528.
Gases
|
Kinetics program for iron(III) catalyzed decomposition of hydrogen peroxide Merrer, Robert J.
A computer program for use in general chemistry has been written in Basic that calculates rate constants and activation energy for the iron(III) catalyzed decomposition of hydrogen peroxide.
Merrer, Robert J. J. Chem. Educ. 1973, 50, 514.
Kinetics |
Rate Law |
Catalysis
|
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
|
Cooking Succulent Roasts Plumb, Robert C.; Davis, Adelle
Allowing a roast to gradually warm to the desired internal temperature produces superior results.
Plumb, Robert C.; Davis, Adelle J. Chem. Educ. 1973, 50, 425.
Consumer Chemistry |
Food Science |
Kinetics |
Equilibrium |
Rate Law |
Applications of Chemistry
|
Cooking Succulent Roasts Plumb, Robert C.; Davis, Adelle
Allowing a roast to gradually warm to the desired internal temperature produces superior results.
Plumb, Robert C.; Davis, Adelle J. Chem. Educ. 1973, 50, 425.
Consumer Chemistry |
Food Science |
Kinetics |
Equilibrium |
Rate Law |
Applications of Chemistry
|
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
|
The definition of the rate of a chemical reaction Canagaratna, S. G.
Most texts take it as obvious that the rate of a reaction may be defined in terms of changes in concentration; this definition is valid only if the reaction takes place without change of volume.
Canagaratna, S. G. J. Chem. Educ. 1973, 50, 200.
Rate Law |
Kinetic-Molecular Theory
|
The determination of dissolved oxygen by the Winkler method. A student laboratory experiment McCormick, Patrick G.
This method is based on the reaction between oxygen and a suspension of manganese(II) hydroxide in a strongly alkaline solution.
McCormick, Patrick G. J. Chem. Educ. 1972, 49, 839.
Water / Water Chemistry |
Aqueous Solution Chemistry |
Gases |
Quantitative Analysis |
Titration / Volumetric Analysis
|
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
|
Demonstrating Avogadro's hypothesis with the molecular dynamics simulator Young, Jay A.; Plumb, Robert C.
The Molecular Dynamics Simulator simulate closely the behaviors predicted by the mathematical descriptions of the kinetic molecular theory.
Young, Jay A.; Plumb, Robert C. J. Chem. Educ. 1972, 49, 709.
Gases |
Kinetic-Molecular Theory
|
The bombardier beetle Plumb, Robert C.; Erickson, Karen L.
The chemistry behind the bombardier beetle's chemical defenses illustrates the principles of reaction rates, catalysis, and laboratory safety.
Plumb, Robert C.; Erickson, Karen L. J. Chem. Educ. 1972, 49, 705.
Applications of Chemistry |
Natural Products |
Rate Law |
Catalysis |
Oxidation / Reduction |
Aromatic Compounds
|
Student flowmeters and an air pollution experiment Kohn, Harold W.
Using glass wool as an absorbent for atmospheric contaminants and three simple devices for measuring flow rates of gases.
Kohn, Harold W. J. Chem. Educ. 1972, 49, 643.
Atmospheric Chemistry |
Gases |
Laboratory Equipment / Apparatus
|
Questions [and] Answers Campbell, J. A.
Eight questions requiring the application of basic principles of chemistry.
Campbell, J. A. J. Chem. Educ. 1972, 49, 624.
Enrichment / Review Materials |
Applications of Chemistry |
Atmospheric Chemistry |
Gases
|
Dissolved oxygen. A relevant experiment for the introductory laboratory Stagg, William R.
Students measure the dissolved oxygen content of water from several natural sources as well as the change in solubility with temperature.
Stagg, William R. J. Chem. Educ. 1972, 49, 427.
Water / Water Chemistry |
Oxidation / Reduction |
Quantitative Analysis |
Solutions / Solvents |
Precipitation / Solubility |
Gases
|
Determination of the molar volume of a gas at standard temperature and pressure. A lecture demonstration Zaborowski, Leon M.
Using massed balloons of measured and corrected volume to determine the molar volume of a gas at standard temperature and pressure.
Zaborowski, Leon M. J. Chem. Educ. 1972, 49, 361.
Gases
|
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
|
Visualization of the atomic absorption of mercury vapor by use of a fluorescent screen Argauer, Robert J.; White, Charles E.
Presents a demonstration to visualize the presence of metallic mercury vapor.
Argauer, Robert J.; White, Charles E. J. Chem. Educ. 1972, 49, 27.
Toxicology |
Gases |
Atomic Properties / Structure
|
Gas Laws, Equilibrium, and the Commercial Synthesis of Nitric acid. A Simple Demonstration Alexander, M. Dale
This demonstration of the commercial production of nitric acid uses a simple apparatus to illustrate a number of basic chemical concepts, including Le Chatelier's principle.
Alexander, M. Dale J. Chem. Educ. 1971, 48, 838.
Synthesis |
Industrial Chemistry |
Acids / Bases |
Gases |
Equilibrium |
Reactions |
Stoichiometry
|
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
|
Concept of empirical temperature for introductory chemistry Ander, Paul
This presentation is used in a freshman course prior to the discussion of the empirical gas laws for dilute gases, i.e., Boyle's Charles', Dalton's etc.,
Ander, Paul J. Chem. Educ. 1971, 48, 325.
Gases
|
Demonstration notes: Spontaneous combustion Johnson, Joseph E.
Modifications or additions to previously published demonstration.
Johnson, Joseph E. J. Chem. Educ. 1970, 47, A439.
Oxidation / Reduction |
Reactions |
Gases |
Transport Properties |
Coordination Compounds
|
Improvement in a Charles' law capillary tube experiment for introductory chemistry laboratory Sawyer, Albert K.
Improving a Charles' law capillary tube experiment for the determination of absolute zero by using a volume-temperature measurement at about -80C using a dry ice/acetone cooling mixture.
Sawyer, Albert K. J. Chem. Educ. 1970, 47, 573.
Gases
|
Prolonging death (in apples) Plumb, Robert C.
Using controlled atmosphere storage to prolong the freshness of vegetables and fruits after they have been harvested.
Plumb, Robert C. J. Chem. Educ. 1970, 47, 518.
Equilibrium |
Kinetics |
Agricultural Chemistry |
Applications of Chemistry |
Gases
|
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
|
Sea-lab experiment Plumb, Robert C.
Illustrating the principles of the kinetic theory of gases.
Plumb, Robert C. J. Chem. Educ. 1970, 47, 175.
Gases |
Kinetic-Molecular Theory
|
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
|
Baby bottles and elementary chemistry Davenport, D. A.
Presents several experiments that rely on baby bottles, including Charles' Law expansion, vapor pressure of volatile liquids, molecular weights of volatile liquids, and closed-atmosphere experiments.
Davenport, D. A. J. Chem. Educ. 1969, 46, 878.
Laboratory Equipment / Apparatus |
Laboratory Management |
Gases |
Liquids |
Oxidation / Reduction
|
An inexpensive vacuum and gas handling system for the freshman laboratory Zuehlke, R. W.; Cartier, P. G.
Presents an inexpensive vacuum and gas handling system for the freshman laboratory.
Zuehlke, R. W.; Cartier, P. G. J. Chem. Educ. 1969, 46, 874.
Laboratory Equipment / Apparatus |
Laboratory Management |
Gases
|
A pseudo-Charles law experiment to teach vapor pressure concepts Sinclair, Dean L.
This deliberately deceptive experiment impresses upon students the basic ideas of vapor pressure and illustrates the scientific method.
Sinclair, Dean L. J. Chem. Educ. 1969, 46, 814.
Gases
|
The noble gases and the periodic table: Telling it like it was Wolfenden, John H.
It is instructive to discover that many great scientists have reported erroneous observations as well as mistaken interpretations of experimental data.
Wolfenden, John H. J. Chem. Educ. 1969, 46, 569.
Gases |
Periodicity / Periodic Table
|
Friday experiments Bissey, Jack E.
Provides data on an unknown gas and asks readers to determine if it is ideal, as well as its molecular weight and chemical formula.
Bissey, Jack E. J. Chem. Educ. 1969, 46, 497.
Gases |
Molecular Properties / Structure
|
The principle of exponential change: Applications in chemistry, biochemistry, and radioactivity Green, Frank O.
Examines the nature of exponential change and its applications to chemistry, biochemistry, and radioactivity, including radioactive decay, enzyme kinetics, colorimetry, spectrophotometry, and first order reaction kinetics.
Green, Frank O. J. Chem. Educ. 1969, 46, 451.
Nuclear / Radiochemistry |
Kinetics |
Enzymes |
Spectroscopy
|
The thermal decomposition of 2,5-dihydrofuran vapor: An experiment in gas kinetics Rubin, Jay A.; Filseth, Stephen V.
Describes an experiment designed to illustrate manipulations with a vacuum system and the conduct of kinetic measurements.
Rubin, Jay A.; Filseth, Stephen V. J. Chem. Educ. 1969, 46, 57.
Kinetics |
Gases
|
Carbon and its inorganic compounds. C. Carbon dioxide Colo, August J.; Alyea, Hubert N.
Demonstrates the production of CO2 from dry ice and limestone and acid.
Colo, August J.; Alyea, Hubert N. J. Chem. Educ. 1968, 45, A326.
Gases |
Synthesis
|
Carbon and its inorganic compounds. B. Carbon monoxide Colo, August J.
Demonstrates the formation of carbon monoxide.
Colo, August J. J. Chem. Educ. 1968, 45, A326.
Gases |
Synthesis
|
Apparatus for determining vapor density Uglum, K. L.; Carson, L. M.; Riley, R. V.
Presents a simplified vapor-density experiment suitable for use as a freshman demonstration or an undergraduate physical chemistry experiment.
Uglum, K. L.; Carson, L. M.; Riley, R. V. J. Chem. Educ. 1968, 45, 203.
Gases |
Laboratory Equipment / Apparatus |
Physical Properties
|
A simple vacuum apparatus for lecture experiments Peterson, L. K.; Ruddy, F. H.
Describes a simple vacuum apparatus and examples of its use in lecture situations.
Peterson, L. K.; Ruddy, F. H. J. Chem. Educ. 1968, 45, 742.
Laboratory Equipment / Apparatus |
Gases |
Liquids |
Physical Properties |
Transport Properties |
Stoichiometry |
Calorimetry / Thermochemistry
|
Chemical queries. Especially for introductory chemistry teachers Young, J. A.; Malik, J. G.; Bolte, John
(1) Is the mole a number or a weight? (2) Is there an easy way to locate a compound by volume and page in Beilstein? (3) What are the stages evident in a gas discharge tube as the pressure of the gas and the voltage are changed? - answer by Bolte
Young, J. A.; Malik, J. G.; Bolte, John J. Chem. Educ. 1968, 45, 718.
Stoichiometry |
Nomenclature / Units / Symbols |
Gases
|
An apparatus for the investigation of Graham's law of effusion Rice, Laurence A.; Chang, James C.
Modification of an earlier apparatus for the investigation of Graham's law of effusion and its applications.
Rice, Laurence A.; Chang, James C. J. Chem. Educ. 1968, 45, 676.
Laboratory Equipment / Apparatus |
Transport Properties |
Gases
|
The revolution in elementary kinetics and freshman chemistry Wolfgang, Richard
New developments in kinetics so fundamentally affect our most elementary conception of chemical change that they must inevitably be reflected in beginning courses in chemistry; includes an outline for freshmen on elementary chemical dynamics.
Wolfgang, Richard J. Chem. Educ. 1968, 45, 359.
Kinetics |
Rate Law |
Mechanisms of Reactions
|
Structure units: Aids in the interpretation of chemical reactions Strong, Laurence E.
the proposal to define structure units as generators of the various properties of a substance has a considerable advantage over the usual definition of a structure unit as the endpoint of some prescribed scheme of subdivision.
Strong, Laurence E. J. Chem. Educ. 1968, 45, 51.
Learning Theories |
Molecular Properties / Structure |
Solids |
Liquids |
Gases
|
The range of validity of Graham's Laws Kirk, A. D.
It is the purpose of this article to discuss effusion, diffusion, and some related processes and to outline the range of validity of Graham's law.
Kirk, A. D. J. Chem. Educ. 1967, 44, 745.
Gases |
Transport Properties
|
Graham's Laws of diffusion and effusion Mason, E. A.; Kronstadt, Barbara
The purpose of this article is to review Graham's laws of diffusion and effusion, offer simple but essentially correct theoretical explanations for both laws, and to present experiments on the diffusion law.
Mason, E. A.; Kronstadt, Barbara J. Chem. Educ. 1967, 44, 740.
Transport Properties |
Gases
|
Accurate measurement of gas volumes by a soap-film method Hello, O.
The measurement of small gas volumes can be greatly improved by using the soap-film apparatus described in this article.
Hello, O. J. Chem. Educ. 1967, 44, 568.
Laboratory Equipment / Apparatus |
Gases
|
Analysis for nitrite by evolution of nitrogen: A general chemistry laboratory experiment Bartlett, J. Kenneth
This experiment involves analysis for the sodium nitrite content of a sodium nitrite-sodium chloride mixture by decomposition to nitrogen while heating in the presence of ammonium chloride solution.
Bartlett, J. Kenneth J. Chem. Educ. 1967, 44, 475.
Gases
|
Capillary tube experiments for introductory chemistry laboratory Gesser, H. D.; Lithown, Caroline; Brattston, D.; Thompson, Ian
Describes the use of a capillary tube to determine how vapor changes with temperature.
Gesser, H. D.; Lithown, Caroline; Brattston, D.; Thompson, Ian J. Chem. Educ. 1967, 44, 387.
Gases |
Phases / Phase Transitions / Diagrams
|
Charles' Law: A general chemistry experiment Haworth, Daniel T.
This paper describes an apparatus that can be used to determine the value of absolute zero.
Haworth, Daniel T. J. Chem. Educ. 1967, 44, 353.
Gases |
Laboratory Equipment / Apparatus
|
An experimental approach to the ideal gas law Breck, W. G.; Holmes, F. W.
It is possible to introduce to students the equation of state, PV = nRT, by an experimental method that demonstrates that PV/T remains constant for a given amount of gas.
Breck, W. G.; Holmes, F. W. J. Chem. Educ. 1967, 44, 293.
Gases
|
Teaching kinetic molecular theory by the factor change method Koons, Lawrence F.
Develops the "factor change method" for teaching kinetic molecular theory and presents examples of its application.
Koons, Lawrence F. J. Chem. Educ. 1967, 44, 288.
Kinetic-Molecular Theory |
Gases
|
The critical temperature: A necessary consequence of gas non-ideality Pilar, F. L.
Illustrates in a non-mathematical fashion that any gas composed of mutually interacting particles of finite volume must exhibit a critical temperature.
Pilar, F. L. J. Chem. Educ. 1967, 44, 284.
Gases
|
VII - Combustion and flame Anderson, Robbin C.
Presents and describes an extensive bibliography on the study of combustion and flames.
Anderson, Robbin C. J. Chem. Educ. 1967, 44, 248.
Oxidation / Reduction |
Reactions |
Gases
|
Hard sphere simulation of statistical mechanical behavior of molecules Plumb, Robert C.
Describes the design and use of a demonstration device to illustrate the kinetic behavior of gases, liquids, and solids.
Plumb, Robert C. J. Chem. Educ. 1966, 43, 648.
Statistical Mechanics |
Gases |
Liquids |
Solids |
Kinetic-Molecular Theory |
Equilibrium |
Phases / Phase Transitions / Diagrams
|
Manometric apparatus for vapor and solution studies Taha, Ahmed A.; Grigsby, Ronald D.; Johnson, James R.; Christian, Sherril D.; Affsprung, Harold E.
Presents a device that can be sued to obtain vapor density and PVT measurements, vapor pressures of solutions and liquids, dew-point pressures and compositions, solubilities of gases in liquids, solubilities of slightly-miscible liquids, equilibrium constants for association reactions in solutions, interactions of vapors and gases with solids, and gas and vapor viscosities.
Taha, Ahmed A.; Grigsby, Ronald D.; Johnson, James R.; Christian, Sherril D.; Affsprung, Harold E. J. Chem. Educ. 1966, 43, 432.
Laboratory Equipment / Apparatus |
Physical Properties |
Solutions / Solvents |
Gases |
Liquids |
Solids
|
The relationship between Avogadro's Principle and the Law of Gay-Lussac Feifer, Nathan
Teaching Avogadro's Principle as an explanation of the phenomena described by Gay-Lussac's Law gives the instructor an opportunity to stress some of the basic assumptions in chemistry and to highlight the logic implicit in Avogadro's reasoning.
Feifer, Nathan J. Chem. Educ. 1966, 43, 411.
Stoichiometry |
Gases
|
IV - Isoelectronic systems Bent, Henry A.
A detailed consideration of the principles of isoelectric systems.
Bent, Henry A. J. Chem. Educ. 1966, 43, 170.
Gases |
Nonmetals |
Covalent Bonding
|
Compressed gas cylinders and cylinder regulators used in laboratories Pinney, George
Presents safety guidelines regarding the use of compressed gas cylinders and cylinder regulators in laboratories.
Pinney, George J. Chem. Educ. 1965, 42, A976.
Laboratory Equipment / Apparatus |
Laboratory Management |
Gases
|
The effect of structure on chemical and physical properties of polymers Price, Charles C.
Suggests using polymers to teach the effect of changes in structure on chemical reactivity, the effect of structure on physical properties, the role of catalysts, and the basic principles of a chain reaction mechanism.
Price, Charles C. J. Chem. Educ. 1965, 42, 13.
Physical Properties |
Molecular Properties / Structure |
Polymerization |
Kinetics |
Reactions |
Catalysis |
Mechanisms of Reactions
|
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
|
"Compounds" (?) of the noble gases prior to 1962 Chernick, Cedric L.
Reviews past efforts to generate compounds of the noble gases.
Chernick, Cedric L. J. Chem. Educ. 1964, 41, 185.
Nonmetals |
Gases
|
The chemistry of the noble gases Hyman, Herbert H.
Summarizes the chemistry of the noble gases and their bond-forming abilities.
Hyman, Herbert H. J. Chem. Educ. 1964, 41, 174.
Gases |
Main-Group Elements |
Covalent Bonding
|
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
|
KineticsEarly and often Campbell, J. A.
Describes an approach to investigating kinetics and its application to the "blue bottle" experiment.
Campbell, J. A. J. Chem. Educ. 1963, 40, 578.
Kinetics |
Equilibrium |
Mechanisms of Reactions
|
Heterogeneous equilibria in general chemistry Grotz, Leonard C.
Presents suggestions for approaching the subject of heterogeneous equilibria in general chemistry.
Grotz, Leonard C. J. Chem. Educ. 1963, 40, 479.
Equilibrium |
Kinetics
|
Hypodermic syringes in quantitative elementary chemistry experiments. Part 2. General chemistry experiments Davenport, Derek A.; Saba, Afif N.
Presents a variety of experiments that make use of hypodermic syringes in quantitative elementary chemistry.
Davenport, Derek A.; Saba, Afif N. J. Chem. Educ. 1962, 39, 617.
Laboratory Equipment / Apparatus |
Gases |
Liquids |
Reactions |
Equilibrium |
Stoichiometry
|
Letters Frigerio, Norman A.; Trotter, Phillip J.
Disposable plastic syringes are found to be more suitable than glass ones to demonstrate P, V, T relationships.
Frigerio, Norman A.; Trotter, Phillip J. J. Chem. Educ. 1962, 39, 594.
Gases
|
Some aspects of chemical kinetics for elementary chemistry Benson, Sidney W.
The author suggests greater efforts to address the issue of kinetics and reaction mechanisms in introductory chemistry.
Benson, Sidney W. J. Chem. Educ. 1962, 39, 321.
Kinetic-Molecular Theory |
Gases |
Kinetics |
Mechanisms of Reactions |
Descriptive Chemistry
|
A simple gas law apparatus Carter, K. N.
The apparatus presented here can be used to verify the ideal gas law, determine the vapor pressure of water at an elevated temperature, or determine the number of moles of dry air under two different sets of conditions for comparison.
Carter, K. N. J. Chem. Educ. 1962, 39, 302.
Laboratory Equipment / Apparatus |
Gases
|
Dalton's law of partial pressures Dutton, Frederic B.
Demonstrates that breaking a sealed ampule of ether in a closed system increases the pressure inside that system.
Dutton, Frederic B. J. Chem. Educ. 1961, 38, A545.
Gases |
Ethers
|
An improved gas generator for elementary chemistry Thiessen, G. W.; Hall, M.
Describes a small-scale adaptation of the Lassieur generator that provides a self-controlled evolution of gas from solid and liquid reagents.
Thiessen, G. W.; Hall, M. J. Chem. Educ. 1961, 38, 19.
Gases |
Laboratory Equipment / Apparatus
|
A constant temperature reaction vessel for the thermal decomposition of solids Prout, E. G.; Herley, P. J.
Describes an apparatus suitable for studying the thermal decomposition of potassium permanganate in high vacuum.
Prout, E. G.; Herley, P. J. J. Chem. Educ. 1960, 37, 643.
Laboratory Equipment / Apparatus |
Solids |
Rate Law |
Kinetics
|
Vapor pressure determination: An elementary experiment Radley, Edward T.
The approximate vapor pressure of low boiling liquids may be estimated by measuring the increase in length of an air column trapped between two short columns of mercury in a uniform diameter tube.
Radley, Edward T. J. Chem. Educ. 1960, 37, 35.
Gases
|
Determination of vapor pressure: A general chemistry laboratory experiment Wolthuis, Enno; Brummel, Roger; Bout, Paul Vanden
Provides a method for obtaining good vapor pressure measurements using simple equipment.
Wolthuis, Enno; Brummel, Roger; Bout, Paul Vanden J. Chem. Educ. 1959, 36, 494.
Gases |
Liquids |
Phases / Phase Transitions / Diagrams
|
A test tube automatic gas generator Alpern, D. K.
A simple design for an automatic gas generator can be used to produce common gases such as hydrogen from zinc and hydrochloric acid.
Alpern, D. K. J. Chem. Educ. 1959, 36, 302.
Laboratory Equipment / Apparatus |
Gases
|
The hydrogen organ Eddy, Robert D.
The hydrogen organ can be used to demonstrate a variety of physical and chemical properties.
Eddy, Robert D. J. Chem. Educ. 1959, 36, 256.
Gases
|
Textbook errors: XX. Miscellanea No. 2 Mysels, Karol J.
Subjects considered include the meaning of "element," the solubility of phenol in carbonate solutions, and the change of vapor pressure with temperature.
Mysels, Karol J. J. Chem. Educ. 1958, 35, 568.
Precipitation / Solubility |
Phenols |
Gases |
Liquids
|
A temperature sensitive stirring rod: Liquefaction of NO2 as a student experiment Eddy, Robert D.; Scholes, Samuel R., Jr.
NO2 is generated from Pb(NO3)2 and collected, condensed, and sealed in a hollow stirring rod, which is then observed in hot, cool, and cold water.
Eddy, Robert D.; Scholes, Samuel R., Jr. J. Chem. Educ. 1958, 35, 527.
Gases |
Phases / Phase Transitions / Diagrams
|
Letters to the editor Saxena, Satish Chandra
The author offers a restatement of Avogadro's law.
Saxena, Satish Chandra J. Chem. Educ. 1956, 33, 188.
Gases |
Stoichiometry
|
Textbook errors: VII. The laws of reaction rates and of equilibrium Mysels, Karol J.
Examines the frequently misplaced emphasis on the rate law of mass action, its fallacious use to prove the existence and form of equilibrium constants, and the occasional confusion of the two concepts.
Mysels, Karol J. J. Chem. Educ. 1956, 33, 178.
Kinetics |
Rate Law |
Equilibrium
|
A simple Charles law experiment Damerell, V. R.
This simple procedure allows students to produce a satisfactory verification of Charles' law.
Damerell, V. R. J. Chem. Educ. 1955, 32, 534.
Gases
|
Textbook errors: III. The solubility of gases in liquids Mysels, Karol J.
Rising temperature is generally said to reduce the solubility of gases in liquids, yet the facts disagree with any such generalization.
Mysels, Karol J. J. Chem. Educ. 1955, 32, 399.
Gases |
Liquids |
Precipitation / Solubility |
Solutions / Solvents
|
Le Châtelier's principle and the equilibrium constant Miller, Arild J.
Many students of chemistry have difficulty in understanding how the position of equilibrium in a gaseous reaction can change when the pressure is altered, in accordance with Le Châtelier's principle, without causing a corresponding variation in the equilibrium constant.
Miller, Arild J. J. Chem. Educ. 1954, 31, 455.
Equilibrium |
Reactions |
Gases
|
A kinetic analogy Lemlich, Robert
This analogy, which clearly demonstrates the principles involved in a first-order reaction, is based on Poiseuille's law for the viscous flow of fluids.
Lemlich, Robert J. Chem. Educ. 1954, 31, 431.
Kinetics
|
Determination of the density of oxygen gas Fiekers, B. A.
The "Oxybomb," a small cartridge of compressed oxygen, is used for determining the density of oxygen gas in laboratory or lecture.
Fiekers, B. A. J. Chem. Educ. 1954, 31, 139.
Gases |
Physical Properties
|
Letters to the editor Lash, M. E.
The author clarifies the definition of critical temperature, which is often stated uncritically in textbooks.
Lash, M. E. J. Chem. Educ. 1954, 31, 102.
Gases |
Phases / Phase Transitions / Diagrams |
Nomenclature / Units / Symbols
|
The kinetic structure of gases Slabaugh, W. H.
Describes a model that illustrates the kinetic properties of gases and ii use to demonstrate the effect of temperature changes on the motion of gas particles.
Slabaugh, W. H. J. Chem. Educ. 1953, 30, 68.
Gases |
Kinetic-Molecular Theory |
Phases / Phase Transitions / Diagrams
|
|
