TIGER

Journal Articles: 171 results
Data Pooling in a Chemical Kinetics Experiment: The Aquation of a Series of Cobalt(III) Complexes  Richard S. Herrick, Kenneth V. Mills, and Lisa P. Nestor
Describes an experiment that introduces students to integrated rate laws, the search for a mechanism that is consistent with chemical and kinetic data, and the concept of activation barriers and their measurement in a curriculum whose pedagogical philosophy makes the laboratory the center of learning for undergraduates in their first two years of instruction.
Herrick, Richard S.; Mills, Kenneth V.; Nestor, Lisa P. J. Chem. Educ. 2008, 85, 1120.
Coordination Compounds |
Kinetics |
Mechanisms of Reactions |
Rate Law |
UV-Vis Spectroscopy
Disorder and Chaos: Developing and Teaching an Interdisciplinary Course on Chemical Dynamics  Steven G. Desjardins
Describes an interdisciplinary course for nonscience majors that introduces ideas about mathematical modeling using examples based on pendulums, chemical kinetics, and population dynamics. Students learn about the nature of measurement and prediction through the use of spreadsheet software for the solution of equations and experimental data collection.
Desjardins, Steven G. J. Chem. Educ. 2008, 85, 1078.
Kinetics |
Mathematics / Symbolic Mathematics |
Nonmajor Courses
A Simple Laboratory Experiment To Determine the Kinetics of Mutarotation of D-Glucose Using a Blood Glucose Meter  Carlos E. Perles and Pedro L. O. Volpe
A simple commercial blood glucose meter is used to follow the kinetics of mutarotation of D-glucose in aqueous solution. The results may be compared with those obtained using an automatic polarimeter.
Perles, Carlos E.; Volpe, Pedro L. O. J. Chem. Educ. 2008, 85, 686.
Aqueous Solution Chemistry |
Bioanalytical Chemistry |
Carbohydrates |
Chirality / Optical Activity |
Enzymes |
Kinetics |
Solutions / Solvents |
Stereochemistry
Physical Chemistry: Thermodynamics (Horia Metiu)
Taylor & Francis, New York, London, 2006. 694 pp. ISBN: 978-0815340911 (paper). $49.95

Physical 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
Reaction Order Ambiguity in Integrated Rate Plots  Joe Lee
This article provides a theoretical and statistical justification for the necessity of monitoring a reaction to a substantial fraction of completion if integrated rate plots plots are to yield unambiguous orders.
Lee, Joe. J. Chem. Educ. 2008, 85, 141.
Chemometrics |
Kinetics |
Rate Law
An Experimental Approach to Teaching and Learning Elementary Statistical Mechanics  Frank B. Ellis and David C. Ellis
This article details demonstrations that show how equilibrium changes with temperature, energy, and entropy and involve exothermic and endothermic reactions, the dynamic nature of equilibrium, and Le Châtelier's principle.
Ellis, Frank B.; Ellis, David C. J. Chem. Educ. 2008, 85, 78.
Equilibrium |
Kinetics |
Statistical Mechanics |
Thermodynamics
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 algorithmicmacroscopic and conceptualmicroscopic levels.
Ashkenazi, Guy. J. Chem. Educ. 2008, 85, 72.
Gases |
Kinetics |
Learning Theories
The Chemistry of Paper Preservation  Henry A. Carter
This article examines the applications of chemistry to paper preservation. The acid-catalyzed hydrolysis of cellulose accounts for the deterioration of paper in library books and other written records. To combat this threat to our written heritage, new permanent papers have been developed that are relatively chemically stable and undergo a very slow rate of deterioration.
Carter, Henry A. J. Chem. Educ. 2007, 84, 1937.
Acids / Bases |
Applications of Chemistry |
Aqueous Solution Chemistry |
Free Radicals |
Gas Chromatography |
HPLC |
pH |
Kinetics |
Rate Law
Visualizing the Transition State: A Hands-on Approach to the Arrhenius Equation  Thomas S. Kuntzleman, Matthew S. Swanson, and Deborah K. Sayers
Pennies and dice are used to simulate the kinetics of two irreversible "reactions" with a hands-on, Monte Carlo approach. Arrhenius plots of the data generated yield activation energies comparable to assigned values and pre-exponential factors close to what would be expected based on the probability of a "reactant" achieving the correct orientation for conversion into "product". A comparison of the values obtained for the pre-exponential factors for the different simulations allows students to semi-quantitatively discuss the orientational requirement that is contained within this factor.
Kuntzleman, Thomas S.; Swanson, Matthew S.; Sayers, Deborah K. J. Chem. Educ. 2007, 84, 1776.
Kinetics |
Rate Law
A Student Laboratory Experiment Based on the Vitamin C Clock Reaction  Ed Vitz
Describes an adaptation of the vitamin C clock reaction to a student laboratory experiment in which the orders with respect to peroxide and iodide, the rate constant, and the activation energy are determined by the method of initial rates.
Vitz, Ed. J. Chem. Educ. 2007, 84, 1156.
Consumer Chemistry |
Kinetics |
Mechanisms of Reactions |
Rate Law
An Inexpensive Kinetic Study: The Reaction of FD&C Red #3 (Erythrosin B) with Hypochlorite  Maher M. Henary and Arlene A. Russell
Students use a desktop visible spectrophotometer to quantitatively follow the rate of disappearance of FD&C Red #3 with hypochlorite. The first-order reaction in both dye and bleach yields simple data that students can easily process and graph using spreadsheet software to obtain the rate constant and the rate law.
Henary, Maher M.; Russell, Arlene A. J. Chem. Educ. 2007, 84, 480.
Dyes / Pigments |
Kinetics |
Rate Law |
UV-Vis Spectroscopy
Applications of Reaction Rate  Kevin Cunningham
This article presents an assignment in which students are to research and report on a chemical reaction whose increased or decreased rate is of practical importance. The assignment is designed to develop and assess a number of valuable skills and understandings, including the ability to write effectively.
Cunningham, Kevin. J. Chem. Educ. 2007, 84, 430.
Catalysis |
Enzymes |
Kinetics |
Rate Law |
Reactions |
Applications of 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 peroxodisulfateiodide 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
An Enzyme Kinetics Experiment Using Laccase for General Chemistry   Yaqi Lin and Patrick M. Lloyd
This article describes the use of laccase, an oxidoreductase enzyme, to study the effects of enzyme catalysts on reaction rates.
Lin, Yaqi; Lloyd, Patrick M. J. Chem. Educ. 2006, 83, 638.
Aldehydes / Ketones |
Bioanalytical Chemistry |
Catalysis |
Enzymes |
Kinetics |
UV-Vis Spectroscopy
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
Simple and Inexpensive Computer Interface to a Durrum Stopped-Flow Apparatus Tested Using the Iron(III)–Thiocyanate Reaction  Craig M. Hoag
Describes a computer interface between a Durrum model 110 stopped-flow apparatus and a LabPro voltage probe using LoggerPro software from Vernier. This probe and software can be used to measure and record data from most instruments normally connected to an oscilloscope or chart recorder.
Hoag, Craig M. J. Chem. Educ. 2005, 82, 1823.
Instrumental Methods |
Kinetics |
Laboratory Computing / Interfacing |
Coordination Compounds |
UV-Vis Spectroscopy
Rotational Mobility in a Crystal Studied by Dielectric Relaxation Spectroscopy. An Experiment for the Physical Chemistry Laboratory  Madalena S. C. Dionísio, Hermínio P. Diogo, J. P. S. Farinha, and Joaquim J. Moura-Ramos
In this article we present a laboratory experiment for an undergraduate physical chemistry course. The purpose of this experiment is the study of molecular mobility in a crystal using the technique of dielectric relaxation spectroscopy. The experiment illustrates important physical chemistry concepts. The background of the experimental technique deals with the concepts of orientational and induced polarization and frequency-dependent relative permittivity (or dielectric constant). The kinetic concepts of temperature-dependent relaxation time, activation energy, and activation entropy are involved in the concept of molecular mobility.
Dionísio, Madalena S. C.; Diogo, Hermínio P.; Farinha, J. P. S.; Moura-Ramos, Joaquim J. J. Chem. Educ. 2005, 82, 1355.
Kinetics |
Phases / Phase Transitions / Diagrams |
Solids |
Crystals / Crystallography
Kinetics of Alcohol Dehydrogenase-Catalyzed Oxidation of Ethanol Followed by Visible Spectroscopy  Kestutis Bendinskas, Christopher DiJiacomo, Allison Krill, and Ed Vitz
A two-week biochemistry experiment was introduced in the second-semester general chemistry laboratory to study the oxidation of ethanol in vitro in the presence of the enzyme alcohol dehydrogenase (ADH). This reaction should pique student interest because the same reaction also occurs in human bodies when alcoholic drinks are consumed. Procedures were developed to follow the biochemical reaction by visible spectroscopy and to avoid specialized equipment. The effect of substrate concentration on the rate of this enzymatic reaction was investigated during the first week. The effects of temperature, pH, the specificity of the enzyme to several substrates, and the enzyme's inhibition by heavy metals were explored during the second week.
Bendinskas, Kestutis; DiJiacomo, Christopher; Krill, Allison; Vitz, Ed. J. Chem. Educ. 2005, 82, 1068.
Enzymes |
Kinetics |
Oxidation / Reduction |
Reactions |
UV-Vis Spectroscopy |
Alcohols |
Biophysical Chemistry |
Food Science
A Modified Demonstration of the Catalytic Decomposition of Hydrogen Peroxide  Carlos Alexander Trujillo
A safer and cheaper version of the popular catalyzed decomposition of hydrogen peroxide demonstration commonly called the Elephants Toothpaste is presented. Hydrogen peroxide is decomposed in the presence of a surfactant by the enzyme catalase producing foam. Catalase has a higher activity compared with the traditional iodide and permits the use of diluted hydrogen peroxide solutions. The demonstration can be made with household products with similar amazing effects.
Trujillo, Carlos Alexander. J. Chem. Educ. 2005, 82, 855.
Catalysis |
Kinetics |
Oxidation / Reduction
A Simple, Inexpensive Water-Jacketed Cuvette for the Spectronic 20  Jonathan E. Thompson and Jason Ting
A simple, inexpensive, water-jacketed cuvette for the Spectronic 20 is described. The cuvette and associated flow system can easily be constructed from materials commonly found in an undergraduate chemistry laboratory. As a demonstration of the cuvette's utility, we used the cuvette for the determination of the activation energy for the reaction between crystal violet and hydroxide ion. However, the cuvette may prove useful in a variety of applications in which a sample must be thermostated within a spectrophotometer.
Thompson, Jonathan E.; Ting, Jason. J. Chem. Educ. 2004, 81, 1341.
Laboratory Equipment / Apparatus |
Kinetics |
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
Promoting Graphical Thinking: Using Temperature and a Graphing Calculator To Teach Kinetics Concepts  José E. Cortés-Figueroa and Deborah A. Moore-Russo
A Calculator-Based Laboratory (CBL) System, a graphing calculator, and a cooling piece of metal are used in a classroom demonstration to teach key concepts of a first-order chemical reaction. This activity promotes graphical thinking and permits student-centered instruction where the students explore concepts and discover how simple mathematical equations model observable facts (data).
Cortés-Figueroa, José E.; Moore-Russo, Deborah A. J. Chem. Educ. 2004, 81, 69.
Kinetics |
Rate Law
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
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
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
Depletion: A Game with Natural Rules for Teaching Reaction Rate Theory  Donald J. Olbris and Judith Herzfeld
Game that reinforces central concepts of rate theory through simulation.
Olbris, Donald J.; Herzfeld, Judith. J. Chem. Educ. 2002, 79, 1232.
Kinetics |
Nonmajor Courses |
Rate Law |
Enrichment / Review Materials |
Catalysis
Factors Affecting Reaction Kinetics of Glucose Oxidase  Kristin A. Johnson
Demonstration based on a biochemical kinetics experiment in which the rate of reaction varies with the enzyme concentration, substrate concentration, substrate used in the reaction, and temperature.
Johnson, Kristin A. J. Chem. Educ. 2002, 79, 74.
Enzymes |
Kinetics |
Proteins / Peptides |
Carbohydrates |
Catalysis |
Rate Law
Putting UV-Sensitive Beads to the Test  Terre Trupp
Explores the temperature behavior of UV-sensitive beads and investigates the effectiveness of sunscreens.
Trupp, Terre. J. Chem. Educ. 2001, 78, 648A.
Atomic Properties / Structure |
Kinetics |
Applications of Chemistry |
Consumer Chemistry |
Photochemistry
Visualizing the Photochemical Steady State with UV-Sensitive Beads (re J. Chem. Educ. 2001, 77, 648A-648B)  Jerry A. Bell
Analysis of the temperature dependence of the color intensity of UV-sensitive beads.
Bell, Jerry A. J. Chem. Educ. 2001, 78, 1594.
Atomic Properties / Structure |
Kinetics |
Photochemistry |
Chemometrics
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
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
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
Simulating Dynamic Equilibria: A Class Experiment  John A. Harrison and Paul D. Buckley
A first-order reversible reaction is simulated on an overhead projector using small coins or discs. Results illustrate how dynamic equilibria are established and allow the introduction of the concept of an equilibrium constant. Le Chtelier's principle is illustrated by further simulations.
Harrison, John A.; Buckley, Paul D. J. Chem. Educ. 2000, 77, 1013.
Equilibrium |
Rate Law |
Reactions
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
Chemistry and Flatulence: An Introductory Enzyme Experiment  John R. Hardee, Tina M. Montgomery, and Wray H. Jones
An enzyme experiment using raffinose family sugars extracted from green split peas as a substrate and the enzymes alpha-galactosidase and sucrase found in Beano. The reaction studied was the hydrolysis of raffinose family sugars to galactose, glucose, and fructose, and the reaction rate was determined using a retail glucometer to measure the concentration of glucose.
Hardee, John R.; Montgomery, Tina M.; Jones, Wray H. J. Chem. Educ. 2000, 77, 498.
Nonmajor Courses |
Enzymes |
Food Science |
Rate Law |
Catalysis |
Applications of Chemistry
Experiments with Aspirin  Londa L. Borer and Edward Barry
Experiments include (i) synthesis, purification, and characterization of aspirin by mp and TLC, (ii) percentage composition of a commercial aspirin tablet by titration, (iii) kinetics of the hydrolysis of aspirin to salicylic acid under various conditions, (iv) synthesis and characterization of copper(II) aspirinate and copper(II) salicylate, and (v) reaction of copper(II) aspirinate in aqueous solution.
Borer, Londa L.; Barry, Edward. J. Chem. Educ. 2000, 77, 354.
Synthesis |
Kinetics |
Drugs / Pharmaceuticals |
Medicinal Chemistry |
Aromatic Compounds
An Experiment to Demonstrate How a Catalyst Affects the Rate of a Reaction  Christine L. Copper and Edward Koubek
This experiment, which is a modified version of the traditional iodine clock reaction, allows students to calculate rates of reaction, orders of reactants, and activation energies. It also lets students discover that to increase a reaction's rate, a catalyst need only provide any additional pathway for the reaction, not necessarily a pathway having a lower activation energy.
Copper, Christine L.; Koubek, Edward. J. Chem. Educ. 1999, 76, 1714.
Catalysis |
Physical Properties |
Rate Law
The Blue Bottle Reaction as a General Chemistry Experiment on Reaction Mechanisms  Steven C. Engerer and A. Gilbert Cook
Using the scientific method (observe, question, hypothesize, experiment, repeat) students propose and test possible reaction mechanisms for the methylene blue-catalyzed oxidation of dextrose with its dramatic color change. Students are led to discover the three-step mechanism through a series of questions.
Engerer, Steven C.; Cook, A. Gilbert. J. Chem. Educ. 1999, 76, 1519.
Aqueous Solution Chemistry |
Kinetics |
Mechanisms of Reactions
Lightstick Kinetics  Charles E. Roser and Catherine L. McCluskey
This experiment determines the energy of activation of the luminescent reaction in a lightstick by measuring the light intensity relative to temperature using Vernier light and temperature sensors, a Texas Instruments CBL interface, and a TI-82/83 graphing calculator.
Roser, Charles E.; McCluskey, Catherine L. J. Chem. Educ. 1999, 76, 1514.
Kinetics |
Photochemistry
Old Rule of Thumb and the Arrhenius Equation  I. A. Leenson
The empirical rule (doubling of the reaction rate upon every 10 increase in temperature) is discussed on the basis of the Arrhenius equation and experimental data. A graph is plotted that shows the applicability limits of the empirical rule in terms of activation energies and temperatures.
Leenson, Ilya A. J. Chem. Educ. 1999, 76, 1459.
Kinetics
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
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
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
A Simple Method To Demonstrate the Enzymatic Production of Hydrogen from Sugar  Natalie Hershlag, Ian Hurley, and Jonathan Woodward
In the experimental protocol described here, it has been demonstrated that the common sugar glucose can be used to produce hydrogen using two enzymes, glucose dehydrogenase and hydrogenase. No sophisticated or expensive hydrogen detection equipment is required-only a redox dye, benzyl viologen, which turns purple when it is reduced. The color can be detected by a simple colorimeter.
Hershlag, Natalie; Hurley, Ian; Woodward, Jonathan. J. Chem. Educ. 1998, 75, 1270.
Enzymes |
Kinetics |
UV-Vis Spectroscopy |
Carbohydrates |
Applications of Chemistry
Why the Arrhenius Equation Is Always in the "Exponentially Increasing" Region in Chemical Kinetic Studies  Harvey F. Carroll
The Arrhenius equation in chemical kinetics, k = Ae-Ea/RT, has, as T gets larger, an inflection point where it changes from an "exponentially increasing" curve to one approaching an asymptote of A. The inflection point occurs at T = Ea/2R. For any activation energy, the inflection point occurs at such a high temperature that chemical kinetic studies would not be possible. Thus, the Arrhenius equation always appears to be exponentially increasing in any chemical kinetic studies of interest.
Carroll, Harvey F. J. Chem. Educ. 1998, 75, 1186.
Kinetics
The Reaction of a Food Colorant with Sodium Hypochlorite: A Student-Designed Kinetics Experiment  Josefina Arce, Rosa Betancourt, Yamil Rivera, and Joan Pijem
The kinetics of the reaction of the food colorant FD&C Blue #1 with sodium hypochlorite (Clorox) is described in a student-designed experimental format. In this format, students are guided- by means of questions- to make decisions regarding concentration of reagents, choice of equipment, and actual laboratory procedures to be followed.
Arce, Josefina; Betancourt-Perez, Rosa; Rivera, Yamil; Pijem, Joan. J. Chem. Educ. 1998, 75, 1142.
Kinetics |
UV-Vis Spectroscopy |
Dyes / Pigments
Chemistry Time: Factors Affecting the Rate of a Chemical Reaction  
This activity can be used to introduce a unit on chemical kinetics, but it is simple enough to be used in a discussion of chemical reactions or experimental methods/procedures during the first weeks of the semester. The activity involves reacting bicarbonate with acid, a reaction with practical applications in everyday life.
J. Chem. Educ. 1998, 75, 1120A.
Kinetics |
Rate Law
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 Kinetics Experiment To Demonstrate the Role of a Catalyst in a Chemical Reaction: A Versatile Exercise for General or Physical Chemistry Students  Christine L. Copper and Edward Koubek
By modifying the iodine clock reaction, students can use the initial rate method to observe the role of a catalyst in a chemical reaction via activation energy calculations and evaluate a proposed mechanism. They can also determine the order with respect to each reactant and the rate constants of the noncatalyzed and catalyzed reactions.
Copper, Christine L.; Koubek, Edward. J. Chem. Educ. 1998, 75, 87.
Catalysis |
Kinetics |
Mechanisms of Reactions
Why Don't Things Go Wrong More Often? Activation Energies: Maxwell's Angels, Obstacles to Murphy's Law  Frank L. Lambert
The micro-complexity of fracturing utilitarian or beautiful objects prevents assigning a characteristic activation energy even to chemically identical artifacts. Nevertheless, a qualitative EACT SOLID can be developed. Its surmounting is correlated with the radical drop in human valuation of an object when it is broken.
Lambert, Frank L. J. Chem. Educ. 1997, 74, 947.
Kinetics |
Nonmajor Courses |
Thermodynamics
Kinetics Studies in a Washing Bottle  John Teggins and Chris Mahaffy
The kinetics of the decomposition of hydrogen peroxide using iodide ion in aqueous solution is studied in sealed completely-filled washing bottles.
Teggins, John; Mahaffy, Chris. J. Chem. Educ. 1997, 74, 566.
Kinetics |
Aqueous Solution Chemistry |
Gases
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 Laboratory Experiment Investigating Different Aspects of Catalase Activity in an Inquiry - Based Approach  Doris R. Kimbrough, Mary Ann Magoun, Meg Langfur
The action of the enzyme catalase on aqueous hydrogen peroxide to generate oxygen gas is a well-established demonstration. Catalase is typically obtained by aqueous extraction of a potato, and the potato extract is mixed together with 3% hydrogen peroxide. The oxygen that is produced can be collected over water. Variations on the procedure can demonstrate the dependence of catalytic activity on temperature or the presence of inhibitors.
Kimbrough, Doris R.; Magoun, Mary Ann; Langfur, Meg . J. Chem. Educ. 1997, 74, 210.
Catalysis |
Rate Law
Resistance Measurement as a Tool for Corrosion Studies  Singh, N. P.; Gupta, S. C.; Sood, B. R.
Procedure for determining the rate of corrosion by measuring changes in the resistance of a thin wire or strip of metal; sample data and analysis included.
Singh, N. P.; Gupta, S. C.; Sood, B. R. J. Chem. Educ. 1995, 72, 465.
Oxidation / Reduction |
Metals |
Rate Law |
Reactions |
Electrochemistry
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 Simple Demonstration of the Effect of Impurities on Melting Point  Hardinger, Steven A.
Demonstration of melting point depression of a substance because of the presence of impurities.
Hardinger, Steven A. J. Chem. Educ. 1995, 72, 250.
Rate Law |
Physical Properties
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
Pictorial Analogies XIII: Kinetics and Mechanism  Fortman, John J.
Pictorial analogies for first order kinetics, the effect of concentration and temperature on reaction rate, and the requirement for proper molecular orientation for reaction.
Fortman, John J. J. Chem. Educ. 1994, 71, 848.
Mechanisms of Reactions |
Rate Law |
Reactions
Chemical Equilibrium in the General Chemistry Course  Fainzilberg, Vladimir E.; Karp, Stewart
The first chapters on chemical equilibrium in first-year college chemistry texts make an "error" in the solution of certain types of equilibria problems.
Fainzilberg, Vladimir E.; Karp, Stewart J. Chem. Educ. 1994, 71, 769.
Equilibrium |
Kinetics
An Oscillating Reaction as a Demonstration of Principles Applied in Chemistry and Chemical Engineering  Weimer, Jeffrey J.
Platinum catalyzed decomposition of methanol.
Weimer, Jeffrey J. J. Chem. Educ. 1994, 71, 325.
Thermodynamics |
Catalysis |
Transport Properties |
Kinetics |
Reactions
Photon-initiated hydrogen-chlorine reaction: A student experiment at the microscale level   Egolf, Leanne M.; Keiser, Joseph T.
This lab offers a way to integrate the principles of thermodynamics and kinetics as well as other valuable instrumental methods.
Egolf, Leanne M.; Keiser, Joseph T. J. Chem. Educ. 1993, 70, A208.
Covalent Bonding |
Ionic Bonding |
Electrochemistry |
Free Radicals |
Microscale Lab |
Thermodynamics |
Kinetics
Photodegradation of methylene blue: Using solar light and semiconductor (TiO2)  Nogueira, Raquel F. P.; Jardim, Wilson F.
An experiment that can be used to introduce or explore concepts such as photochemistry, semiconductors, and kinetics.
Nogueira, Raquel F. P.; Jardim, Wilson F. J. Chem. Educ. 1993, 70, 861.
Semiconductors |
Photochemistry |
Kinetics |
Catalysis |
MO Theory
Using the electrician's multimeter in the chemistry teaching laboratory: Part 1. Colorimetry and thermometry experiments  Andres, Roberto T.; Sevilla, Fortunato, III
The multimeter could be a very useful instrument for the chemistry laboratory bench. In this paper, the versatility of the multimeter in the chemistry teaching laboratory is demonstrated.
Andres, Roberto T.; Sevilla, Fortunato, III J. Chem. Educ. 1993, 70, 514.
Laboratory Equipment / Apparatus |
Equilibrium |
Stoichiometry |
Kinetics |
Calorimetry / Thermochemistry
Monitoring self-association of a hydrophobic peptide with high performance liquid chromatography: An undergraduate kinetic experiment using the antibiotic gramicidin A  Braco, Lorenzo; Ba, M. Carmen; Abad, Concepcin
The authors propose a kinetic experiment that uses high performance liquid chromatography to determine the rate and equilibrium constants in a very simple manner, and separate the molecular species under study.
Braco, Lorenzo; Ba, M. Carmen; Abad, Concepcin J. Chem. Educ. 1992, 69, A113.
HPLC |
Kinetics |
Proteins / Peptides |
Rate Law |
Equilibrium
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
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
Applications of Maxwell-Boltzmann distribution diagrams.  Peckham, Gavin D.; McNaught, Ian J.
Although Maxwell-Boltzmann distribution diagrams are intuitively appealing, care must be taken to avoid several common errors and misconceptions.
Peckham, Gavin D.; McNaught, Ian J. J. Chem. Educ. 1992, 69, 554.
Thermodynamics |
Rate Law |
Catalysis
A study of some 2-chloro-2-methylpropane kinetics using a computer interface  Allen, Anthony; Haughey, Adam J.; Hernandez, Yolanda; Ireton, Scot
Examining the effects of a few variables on the rate of a chemical reaction using specialized software.
Allen, Anthony; Haughey, Adam J.; Hernandez, Yolanda; Ireton, Scot J. Chem. Educ. 1991, 68, 609.
Kinetics |
Rate Law |
Acids / Bases |
Laboratory Computing / Interfacing
A demonstration illustrating the factors determining rates of chemical reactions   Holmes, L. H., Jr.
This demonstration qualitatively illustrates factors determining reaction rates for first-year chemistry students.
Holmes, L. H., Jr. J. Chem. Educ. 1991, 68, 501.
Rate Law |
Kinetics
Ants and chemical kinetics  Myers, R. Thomas
Data regarding the speed of ants at various temperatures are amenable to standards treatment on chemical kinetics.
Myers, R. Thomas J. Chem. Educ. 1990, 67, 761.
Kinetics |
Rate Law
A simple second-order kinetics experiment  Weiss, Hilton M.; Touchette, Kim
The reaction studied in this experiment is the (reversible) dimerization of 2,5-dimethyl-3,4-diphenylcyclopentadienone; the monomer is colored while the dimer is not, so monitoring the reaction with a simple spectrophotometer provides the concentration of the monomer and therefore the rate of its disappearance.
Weiss, Hilton M.; Touchette, Kim J. Chem. Educ. 1990, 67, 707.
Kinetics |
Spectroscopy |
Aromatic Compounds
A bromate clock reaction: The formation of purple tris(diphosphato)manganate(III)  Rich, Ronald L.; Noyes, Richard M.
Bromate is used to oxidize nearly colorless Mn(II) to a deep purple complex of Mn(III).
Rich, Ronald L.; Noyes, Richard M. J. Chem. Educ. 1990, 67, 606.
Reactions |
Oxidation / Reduction |
Kinetics
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
Wet labs, computers, and spreadsheets  Durham, Bill
The following is a description of some commonly encountered experiments that have been modified for computerized data acquisition.
Durham, Bill J. Chem. Educ. 1990, 67, 416.
Laboratory Computing / Interfacing |
Nuclear / Radiochemistry |
Titration / Volumetric Analysis |
Calorimetry / Thermochemistry |
Kinetics |
Electrochemistry
Two easy chemical rate experiments   Garver, Emerson E.
One can use the spectrophotometer to investigate the rates of colored chemical reactions in solution.
Garver, Emerson E. J. Chem. Educ. 1990, 67, 183.
Rate Law |
Spectroscopy
Polarized light and rates of chemical reactions  Weir, John J.
This experiment provides the opportunity to introduce the principles of reaction kinetics, polarized light, and the chemistry of optically active compounds; the rate of the acid-catalyzed hydrolysis of sucrose to glucose and fructose is determined.
Weir, John J. J. Chem. Educ. 1989, 66, 1035.
Rate Law |
Kinetics |
Chirality / Optical Activity |
Carboxylic Acids
Catalysis: New reaction pathways not just a lowering of the activation energy  Haim, Albert
The explanation that the increased rate associated with a catalyzed reaction is the result of a lowering of the activation energy cannot always be correct.
Haim, Albert J. Chem. Educ. 1989, 66, 935.
Catalysis |
Rate Law
Kinetics of the fading of phenolphthalein in alkaline solution  Nicholson, Lois
The fading of phenolphthalein in alkaline solution can serve as the basis for an experiment illustrating first-order kinetics.
Nicholson, Lois J. Chem. Educ. 1989, 66, 725.
Acids / Bases |
Kinetics
Chemical principles for the introductory laboratory, CHM 384 (Johnson, James F.)  Wegner, Carol
A comprehensive review of the title program which overviews basic techniques and concepts presented in introductory laboratory courses. Topics include: titration, equilibrium, Ksp, solubility, Beer's law, coordination complexes and first-order rates of reaction.
Wegner, Carol J. Chem. Educ. 1988, 65, A47.
Acids / Bases |
Titration / Volumetric Analysis |
UV-Vis Spectroscopy |
Equilibrium |
Solutions / Solvents |
Coordination Compounds |
Kinetics
The study of a simple redox reaction as an experimental approach to chemical kinetics  Elias, Horst; Zipp, Arden P.
The authors present a kinetics experiment based on the oxidation of iodide ions that, like the iodine clock, is quick and easy to perform but has the advantage of being followed directly rather than indirectly.
Elias, Horst; Zipp, Arden P. J. Chem. Educ. 1988, 65, 737.
Kinetics |
Reactions |
Rate Law
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
Computer-Assisted Blackboard (Soltzberg, L. J.)  Kruger, J. D.
8-disk set of programs (Apple II) designed to help a lecturer illustrate gas laws, the Rutherford atomic model, quantization in a Bohr atom, wave-functions and orbitals, heat and changes in state, kinetics and simple reaction mechanisms, equilibrium, acid-base reactions, and titrations.
Kruger, J. D. J. Chem. Educ. 1987, 64, A135.
Acids / Bases |
Gases |
Atomic Properties / Structure |
Phases / Phase Transitions / Diagrams |
Kinetics |
Mechanisms of Reactions |
Equilibrium |
Titration / Volumetric Analysis
Coupled oscillations  Onwood, D. P.
Demonstrating coupled oscillations using pendulums.
Onwood, D. P. J. Chem. Educ. 1987, 64, 351.
Kinetics
Kinetics and mechanism of the iodine azide reaction: A videotaped experiment  Haight, Gilbert P.; Jones, Loretta L.
A clock reaction suitable for videotaping and presenting to a large lecture class of general chemistry for analysis.
Haight, Gilbert P.; Jones, Loretta L. J. Chem. Educ. 1987, 64, 271.
Kinetics |
Mechanisms of Reactions |
Rate Law
Windowsill kinetics: A spectrophotometric study of the photochromism of mercury dithizonate  Petersen, Richard L.; Harris, Gaylon L.
Mercury dithizonate undergoes a color change from orange to an intense royal blue upon irradiation with visible light.
Petersen, Richard L.; Harris, Gaylon L. J. Chem. Educ. 1985, 62, 802.
Photochemistry |
Spectroscopy |
Kinetics |
Coordination Compounds |
Raman Spectroscopy
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
Change in concentration with time  Umland, Jean B.
Shows how the rate of a reaction is fast at first and then gradually decreases to zero when one reactant has been used up.
Umland, Jean B. J. Chem. Educ. 1985, 62, 153.
Solutions / Solvents |
Kinetics |
Rate Law
Thermodynamic changes, kinetics, equilibrium, and LeChatelier's principle  Hansen, Robert C.
A series of demonstrations in which water in beakers and the flow of water between beakers is used to represent the components of an exothermic chemical reaction and the flow and quantity of thermal energy involved in chemical changes.
Hansen, Robert C. J. Chem. Educ. 1984, 61, 804.
Equilibrium |
Kinetics |
Thermodynamics
A demonstration of the effect of temperature on reaction rate (the authors reply)  Boring, Wayne C.; McMillan, Ernest
Addresses problems identified with their demonstration / experiment.
Boring, Wayne C.; McMillan, Ernest J. Chem. Educ. 1984, 61, 744.
Kinetics |
Rate Law
A demonstration of the effect of temperature on reaction rate  Gupta, Y. K.; Mishra, S. K.
Problems with the experiment cited.
Gupta, Y. K.; Mishra, S. K. J. Chem. Educ. 1984, 61, 744.
Kinetics |
Rate Law
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
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
Influence of temperature and catalyst on the decomposition of potassium chlorate in a simple DTA apparatus  Wiederholt, Erwin
The authors describe the use of a simple DTA-apparatus in demonstrating the catalytic effects of MnO2 and Al2O3 on the decomposition temperature of KClO3.
Wiederholt, Erwin J. Chem. Educ. 1983, 60, 431.
Kinetics |
Instrumental Methods |
Catalysis |
Reactions |
Rate Law
A safe and simple demonstration of the effect of temperature on reaction rate  Boring, Wayne C.; McMillan, Ernest T.
The demonstration described here utilizes a safe and familiar reaction to illustrate the concept of reaction rate to students.
Boring, Wayne C.; McMillan, Ernest T. J. Chem. Educ. 1983, 60, 414.
Kinetics |
Reactions
Getting a "bang" out of chemical kinetics  Hague, George R., Jr.
The kinetics demonstration described in this note has attracted as many as 15,000people to come and watch.
Hague, George R., Jr. J. Chem. Educ. 1983, 60, 355.
Kinetics
The kinetics of photographic development: A general chemistry experiment  Byrd, J. E.; Perona, M. J.
An experiment that uses black and white photographic equipment to illustrate the determination of reaction rate, kinetic order of reactant, and activation energy.
Byrd, J. E.; Perona, M. J. J. Chem. Educ. 1982, 59, 335.
Kinetics |
Applications of Chemistry |
Photochemistry |
Rate Law
Let's get the heck out of here!  White, Alvan D.
A football stadium is used to explain rate-determining steps.
White, Alvan D. J. Chem. Educ. 1981, 58, 645.
Rate Law |
Kinetics
"Scientific method" through laboratory experience  Hanson, Allen L.
The laboratory presented here will give the students some practice in scientific laboratory habits and general scientific habits of mind.
Hanson, Allen L. J. Chem. Educ. 1981, 58, 434.
Kinetics
Temperature effect on reaction rates   Eliason, Robert; McMahon, Terence
A demonstration has been developed which nicely illustrates the temperature effect on reaction rates and the general rule relating temperature increases with rate increases.
Eliason, Robert; McMahon, Terence J. Chem. Educ. 1981, 58, 354.
Kinetics |
Reactions
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
An introductory level kinetics investigation  McGarvey, J. E. B.; Knipe, A. C.
A kinetic study of the hydrolysis of 3-bromo-3-phenylpropanoic acid.
McGarvey, J. E. B.; Knipe, A. C. J. Chem. Educ. 1980, 57, 155.
Kinetics |
Rate Law |
Mechanisms of Reactions
Rossini, William Tell and the iodine clock reaction: A lecture demonstration  Brice, L. K.
The iodine clock reaction is timed to coincide with three portions of the William Tell Overture.
Brice, L. K. J. Chem. Educ. 1980, 57, 152.
Reactions |
Kinetics |
Rate Law
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
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
The hydrolysis of p-nitrophenyl beta-gIucoside: An undergraduate experiment on the effect of temperature on reaction rate  Schram, Alfred. C.
The intensely colored p-nitrophenolate ion formed during basic hydrolysis allows a quick and convenient determination of the amount of product formed.
Schram, Alfred. C. J. Chem. Educ. 1979, 56, 351.
Kinetics |
Rate Law
Rates of reaction - Analogies  Smith, Douglas D.
Demonstrations of / analogies for zero- and first-order reactions.
Smith, Douglas D. J. Chem. Educ. 1979, 56, 47.
Rate Law |
Kinetics
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 Demonstration of burning magnesium and dry ice  Driscoll, Jerry A.
This demonstration is a new, exciting approach to an older demonstration.
Driscoll, Jerry A. J. Chem. Educ. 1978, 55, 450.
Thermodynamics |
Kinetics |
Reactions
The Landolt, "Old Nassau", and variant reactions   Moss, Arthur
Instructions for a modification to the classic "iodine clock" reaction.
Moss, Arthur J. Chem. Educ. 1978, 55, 244.
Kinetics |
Reactions
Collision theory  Myers, Richard S.
The question presented here can be employed in general or physical chemistry courses.
Myers, Richard S. J. Chem. Educ. 1978, 55, 243.
Chemometrics |
Thermodynamics |
Kinetics
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
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
Faster than a speeding bullet. A freshman kinetics experiment  Cassen, T.
A description of a "clock" experiment that is useful for a freshman level experiment dealing with kinetics.
Cassen, T. J. Chem. Educ. 1976, 53, 197.
Kinetics
Coffee cup kinetics. A general chemistry experiment  Birk, James P.
This laboratory activity attempts to fill the void of a lack of kinetics experiments in general chemistry.
Birk, James P. J. Chem. Educ. 1976, 53, 195.
Kinetics
A simple general chemistry kinetics experiment  Gellender, Martin
The oxidation of iodide ion by persulfate provides a gradual and clearly distinguishable appearance of color as the reaction proceeds.
Gellender, Martin J. Chem. Educ. 1975, 52, 806.
Kinetics |
Rate Law |
Reactions |
Oxidation / Reduction
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
A stabilized linear direct reading conductance apparatus. The solvolysis of t-butyl chloride  Cyr, T.; Prudhomme, J.; Zador, M.
A simple ac conductivity apparatus for experiments in chemical kinetics is described; the instrument is sufficiently reliable that it can be used by first year students and assembled in a few hours.
Cyr, T.; Prudhomme, J.; Zador, M. J. Chem. Educ. 1973, 50, 572.
Laboratory Equipment / Apparatus |
Instrumental Methods |
Electrochemistry |
Kinetics
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
An oscillating iodine clock  Briggs, Thomas S.; Rauscher, Warren C.
An oscillating iodine clock reaction that gives striking cyclic changes from colorless to gold to blue using simple reagents.
Briggs, Thomas S.; Rauscher, Warren C. J. Chem. Educ. 1973, 50, 496.
Reactions |
Kinetics
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
Effect of temperature on reaction rate  Simon, J.
The reaction of aluminum in HCl.
Simon, J. J. Chem. Educ. 1972, 49, A85.
Rate Law |
Reactions
Durable chrome plating  Plumb, Robert C.; Saur, Roger L.
How chrome plating works to protect bumpers from corrosion.
Plumb, Robert C.; Saur, Roger L. J. Chem. Educ. 1972, 49, 626.
Electrochemistry |
Oxidation / Reduction |
Applications of Chemistry |
Kinetics
Durable chrome plating  Plumb, Robert C.; Saur, Roger L.
How chrome plating works to protect bumpers from corrosion.
Plumb, Robert C.; Saur, Roger L. J. Chem. Educ. 1972, 49, 626.
Electrochemistry |
Oxidation / Reduction |
Applications of Chemistry |
Kinetics
The hydroxylaminolysis of penicillin G. A kinetic experiment  Stuckwisch, C. G.
Penicillin reacts with hydroxylamine to yield a hydroxamic acid, which gives a colored complex with iron (III).
Stuckwisch, C. G. J. Chem. Educ. 1972, 49, 539.
Kinetics |
Rate Law |
Titration / Volumetric Analysis
Passage of fruit flies through a hole. A model for a reversible chemical reaction  Runquist, Elizabeth A.; Runquist, Olaf
The passage of fruit flies through a single orifice provides an excellent model for illustrating the principles of equilibrium and chemical dynamics; the results are found to be temperature dependent and reproducible.
Runquist, Elizabeth A.; Runquist, Olaf J. Chem. Educ. 1972, 49, 534.
Reactions |
Equilibrium |
Kinetics |
Rate Law
Aquation of tris-(1,10-phenanthroline) iron(II) in acid solution. A kinetics experiment  Twigg, Martyn V.
The aquation of tris-(1,10-phenanthroline) iron(II) in acid solution is a reaction for which reliable kinetic data are available and it has an easily measured rate at accessible temperatures.
Twigg, Martyn V. J. Chem. Educ. 1972, 49, 371.
Kinetics |
Rate Law
The color blind traffic light. An undergraduate kinetics experiment using an oscillating reaction  Lefelhocz, John F.
This kinetics experiment involves the student with a qualitative study of the influence of chemical and physical variables on the rate of a specific reaction.
Lefelhocz, John F. J. Chem. Educ. 1972, 49, 312.
Kinetics |
Reactions |
Rate Law
Programmable calculators. Simulated experiments  Runquist, O.; Olsen, Rodney; Snadden, Bruce
Describes how titration and reaction rate experiments can be simulated on a programmable calculator.
Runquist, O.; Olsen, Rodney; Snadden, Bruce J. Chem. Educ. 1972, 49, 265.
Acids / Bases |
Titration / Volumetric Analysis |
Quantitative Analysis |
Rate Law |
Kinetics |
pH
Computer program for the treatment of data for a kinetic study of the persulfate-iodide clock reaction  Lyndrup, Mark L.
Notes the availability of a BASIC program designed to aid students in the treatment of data collected for a kinetic study of the clock reaction between the persulfate and iodide ions.
Lyndrup, Mark L. J. Chem. Educ. 1972, 49, 30.
Kinetics |
Reactions |
Rate Law
A demonstration of enzyme activity for the "Sceptical Chymist"  Fried, Rainer; Howse, Margaret
A simple laboratory or demonstration that illustrates the nature and fundamental properties of enzymes through a color change.
Fried, Rainer; Howse, Margaret J. Chem. Educ. 1971, 48, 847.
Enzymes |
Rate Law
A study of the physical and chemical rates of CaCO3 dissolution in HCl  Bassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, Ben
The authors describe the experimental procedure and a discussion of results for a study of the physical and chemical rates of CaCO3 dissolution in HCl.
Bassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, Ben J. Chem. Educ. 1971, 48, 327.
Acids / Bases |
Kinetics |
Reactions |
Rate Law
Miscellaneous  Alyea, Hubert N.
These twelve overhead projection demonstrations include rates of reactions, clock reactions, the effect of temperature and the presence of a catalyst on the decomposition of hydrogen peroxide, the relationship between viscosity and temperature, equilibria, solubility product, and the common ion effect.
Alyea, Hubert N. J. Chem. Educ. 1970, 47, A437.
Oxidation / Reduction |
Kinetics |
Rate Law |
Reactions |
Acids / Bases |
Catalysis |
Equilibrium |
Precipitation / Solubility
Hydrolysis of benzenediazonium ion  Sheats, John E.; Harbison, Kenneth G.
Presents a more convenient approach to studying the kinetics of the hydrolysis of benzenediazonium ion.
Sheats, John E.; Harbison, Kenneth G. J. Chem. Educ. 1970, 47, 779.
Aromatic Compounds |
Nucleophilic Substitution |
Kinetics
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
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
Definition of reaction rate and the steady state assumption  Rasiel, Yecheskel; Freeman, Wade A.
Clarifies the definition of reaction rate and the steady state assumption.
Rasiel, Yecheskel; Freeman, Wade A. J. Chem. Educ. 1970, 47, 159.
Rate Law |
Reactions
Chemical queries. Especially for introductory chemistry teachers  Young, J. A.; Malik, J. G.; House, J. E., Jr.; Campbell, J. A.
(1) When is the rule valid that the rate of reaction approximately doubles with a ten-degree temperature rise? - answer by House. (2) On the colors of transition metal complexes. (3) On an electrolysis experiment in which an acid solution is used to minimize the hydrolysis of Cu 2+. - answer by Campbell.
Young, J. A.; Malik, J. G.; House, J. E., Jr.; Campbell, J. A. J. Chem. Educ. 1969, 46, 674.
Rate Law |
Kinetics |
Transition Elements |
Coordination Compounds |
Atomic Properties / Structure |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Acids / Bases
The law of mass action  Berline, Steven; Bricker, Clark
It is the purpose of this paper to present a derivation of the Law of Mass Action that should have meaning and could be used at an elementary level.
Berline, Steven; Bricker, Clark J. Chem. Educ. 1969, 46, 499.
Equilibrium |
Rate Law |
Kinetics
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
From stoichiometry and rate law to mechanism  Edwards, John O.; Greene, Edward F.; Ross, John
Examines the rules used by chemists as guidelines in developing mechanisms from stoichiometric and rate law observations.
Edwards, John O.; Greene, Edward F.; Ross, John J. Chem. Educ. 1968, 45, 381.
Stoichiometry |
Rate Law |
Kinetics |
Mechanisms of Reactions |
Equilibrium |
Reactive Intermediates
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
Instantaneous precipitation from homogeneous solution  Hiskey, C. F.; Cantwell, F. F.
Procedure for the iodine clock reaction.
Hiskey, C. F.; Cantwell, F. F. J. Chem. Educ. 1967, 44, A727.
Precipitation / Solubility |
Aqueous Solution Chemistry |
Kinetics
Alcohols to alkyl halides: A kinetics experiment for elementary chemistry courses  Cooley, J. H.; McCown, J. D.; Shill, R. M.
The rate measurement in this procedure is accomplished by direct observation of the change in length or volume of the insoluble layer of an alkyl bromide that is formed from a mixture of alcohol, hydrobromic acid, and sulfuric acid.
Cooley, J. H.; McCown, J. D.; Shill, R. M. J. Chem. Educ. 1967, 44, 280.
Alcohols |
Synthesis |
Kinetics |
Rate Law
The dissolution of tin in solutions of iodine  Davies, J. F.; Trotman-Dickenson, A. F.
The progress of this reaction can be followed by the loss of weight of a tin disc.
Davies, J. F.; Trotman-Dickenson, A. F. J. Chem. Educ. 1966, 43, 483.
Solutions / Solvents |
Precipitation / Solubility |
Kinetics |
Gravimetric Analysis
Acid-catalyzed hydrolysis of sucrose: A student study of a reaction mechanism  Dawber, J. G.; Brown, D. R.; Reed, R. A.
By extending the experimental work in a kinetic study of the hydrolysis of sucrose, the beginning student in chemistry can gather some insight into the mechanism of the reaction.
Dawber, J. G.; Brown, D. R.; Reed, R. A. J. Chem. Educ. 1966, 43, 34.
Kinetics |
Mechanisms of Reactions |
Reactions |
Carbohydrates
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
A new clock reaction preparation of dicinnamalacetone  King, L. Carroll; Ostrum, G. Kenneth
Presents a new clock reaction preparation of dicinnamalacetone.
King, L. Carroll; Ostrum, G. Kenneth J. Chem. Educ. 1964, 41, A139.
Reactions |
Kinetics |
Rate Law
Infrared spectrometry to study second order reaction kinetics  Gastambide, B.; Blanc, J.; Allamagny, Y.
The change studied is a synthesis reaction between menthol and phenyl isocyanate.
Gastambide, B.; Blanc, J.; Allamagny, Y. J. Chem. Educ. 1964, 41, 613.
Spectroscopy |
IR Spectroscopy |
Reactions |
Kinetics |
Synthesis
The hydration of carbon dioxide: A double clock experiment  Jones, P.; Haggett, Max L.; Longridge, Jethro L.
This extension of the "Soda Water Clock" experiment provides a quantitative kinetics investigation.
Jones, P.; Haggett, Max L.; Longridge, Jethro L. J. Chem. Educ. 1964, 41, 610.
Reactions |
Rate Law |
Kinetics |
pH |
Acids / Bases |
Aqueous Solution Chemistry
A kinetics experiment for first year chemistry  Shaefer, William P.
The exchange of iodine atoms between organic and inorganic iodides serves as a kinetics experiment for first year chemistry.
Shaefer, William P. J. Chem. Educ. 1964, 41, 558.
Kinetics |
Isotopes |
Rate Law
The oxidation of iodide ion by persulfate ion  Moews, P. C., Jr.; Petrucci, R. H.
Presents the oxidation of iodide ion by persulfate ion as an ideal reaction to study as part of an experiment on kinetics.
Moews, P. C., Jr.; Petrucci, R. H. J. Chem. Educ. 1964, 41, 549.
Oxidation / Reduction |
Reactions |
Kinetics |
Rate Law
A second order kinetics experiment  Teerlink, Wilford J.; Asay, Jeanette; Sugihara, James M.
Investigates the nucleophilic displacement reaction of ethyl p-toluenesulfonate by iodide in acetone.
Teerlink, Wilford J.; Asay, Jeanette; Sugihara, James M. J. Chem. Educ. 1964, 41, 161.
Kinetics |
Nucleophilic Substitution
Colorimetric chemical kinetics experiment  Corsaro, Gerald
This article describes an experiment in which a photocolorimetric technique is employed to follow a bimolecular reaction rate; the reactants are crystal violet and the hydroxide ion.
Corsaro, Gerald J. Chem. Educ. 1964, 41, 48.
Kinetics |
Rate Law |
Reactions
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
KineticsEarly 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
A simple kinetics experiment for general chemistry laboratory  Cone, W. H.; Hermens, R. A.
This simple kinetics experiment examines the oxidation of benzoic acid by potassium peroxodisulfate in the presence of catalytic amounts of silver ion.
Cone, W. H.; Hermens, R. A. J. Chem. Educ. 1963, 40, 421.
Kinetics |
Rate Law |
Oxidation / Reduction |
Catalysis
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 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
Determination of reaction rates with an A.C. conductivity bridge: A student experiment  Chesick, J. P.; Patterson, A., Jr.
Describes a quantitative experiment in chemical kinetics suitable for advanced freshmen or physical chemistry; it involves a study of the solvolysis of tertiary butyl chloride by means of conductance measurements.
Chesick, J. P.; Patterson, A., Jr. J. Chem. Educ. 1960, 37, 242.
Conductivity |
Kinetics |
Rate Law
Use of radioisotopes in the college chemistry laboratory  Phillips, David; Maybury, Robert H.
Provides experiments and experiences working with constructed Geiger counters and radioisotopes.
Phillips, David; Maybury, Robert H. J. Chem. Educ. 1959, 36, 133.
Nuclear / Radiochemistry |
Isotopes |
Instrumental Methods |
Qualitative Analysis |
Kinetics
The formaldehyde clock reaction  Barrett, Richard L.
The formaldehyde clock reaction has some advantages over the familiar iodine clock and deserves to be better known.
Barrett, Richard L. J. Chem. Educ. 1955, 32, 78.
Reactions |
Kinetics |
Rate Law |
Aldehydes / Ketones
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