| Journal Articles: 30 results |
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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
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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
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Textbook Deficiencies: Ambiguities in Chemical Kinetics Rates and Rate Constants Keith T. Quisenberry and Joel Tellinghuisen
Recommends that textbook authors make it clear that (i) the reaction rate and rate constant cannot be defined unambiguously without explicitly stating the reaction for which they apply and therefore (ii) the relation between the half-life, which is a physical property of the reaction system, and the rate constant depends upon how the reaction is written.
Quisenberry, Keith T.; Tellinghuisen, Joel. J. Chem. Educ. 2006, 83, 510.
Kinetics |
Rate Law
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An Interactive Classroom Activity Demonstrating Reaction Mechanisms and Rate-Determining Steps Laura D. Jennings and Steven W. Keller
An interactive classroom activity is described that allows visualization of microscopic reaction mechanisms via the macroscopic process of unwrapping and eating chocolate candies.
Jennings, Laura D.; Keller, Steven W. J. Chem. Educ. 2005, 82, 549.
Reactions |
Rate Law |
Kinetics
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A Modular Laser Apparatus for Polarimetry, Nephelometry, and Fluorimetry in General Chemistry Scott A. Darveau, Jessica Mueller, April Vaverka, Cheri Barta, Anthony Fitch, Jessica Jurzenski, and Yvonne Gindt
We present an apparatus suitable for multiple uses in the general chemistry laboratory including polarimetry, fluorescence, and nephelometry. The open design of the instrument also decreases the chance that students will contract the "black-box syndrome" that seems to develop when using instruments that only provide the final data in an experiment without showing how the measurements are obtained.
Darveau, Scott A.; Mueller, Jessica; Vaverka, April; Barta, Cheri; Fitch, Anthony; Jurzenski, Jessica; Gindt, Yvonne. J. Chem. Educ. 2004, 81, 401.
Fluorescence Spectroscopy |
Kinetics |
Laboratory Equipment / Apparatus |
Lasers |
Spectroscopy |
Proteins / Peptides |
Water / Water Chemistry
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Don't Be Tricked by Your Integrated Rate Plot Edward Urbansky
Reply to comments on original article.
Urbansky, Edward. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
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Don't Be Tricked by Your Integrated Rate Plot: Reaction order Ambiguity Sue Le Vent
Integrated rate equations (for constant reaction volume) may be given in terms of relative reactant concentration, C (= concentration/initial concentration) and relative time, T (= time/half-life); in these forms, the equations are independent of rate constants and initial concentrations.
Le Vent, Sue. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
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Don't Be Tricked by Your Integrated Rate Plot: Pitfalls of Using Integrated Rate Plots Gabor Lente
Problems with linearizing the integrated rate law.
Lente, Gabor. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
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Don't Be Tricked by Your Integrated Rate Plot: Pitfalls of Using Integrated Rate Plots Gabor Lente
Problems with linearizing the integrated rate law.
Lente, Gabor. J. Chem. Educ. 2004, 81, 32.
Kinetics |
Mechanisms of Reactions |
Chemometrics
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Flipping Pennies and Burning Candles: Adventures in Kinetics Michael J. Sanger
Activity in which students collect data to determine whether two processes, flipping pennies and burning candles, follow zeroth- or first-order rate laws.
Sanger, Michael J. J. Chem. Educ. 2003, 80, 304A.
Kinetics |
Rate Law
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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
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Rate Law Determination of Everyday Processes Michael J. Sanger, Russell A. Wiley Jr., Erwin W. Richter, and Amy J. Phelps
Laboratory to determine whether burning a candle and flipping pennies follow zero-, first-, or second-order rate laws.
Sanger, Michael J.; Wiley, Russell A., Jr.; Richter, Erwin W.; Phelps, Amy J. J. Chem. Educ. 2002, 79, 989.
Kinetics |
Rate Law
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Modeling Chemical Processes in Seawater Aquaria to Illustrate Concepts in Undergraduate Chemistry Gordan Grguric
This paper describes three exercises which can be used in a variety of undergraduate chemistry curricula: (i) determining the salts and their amounts needed to prepare a given volume of artificial seawater, (ii) modeling aqueous carbonate equilibria, to calculate pH and alkalinity shifts through additions of chemicals, and (iii) modeling chemical kinetics involved in aqueous ozone-bromine reactions, to predict the type and extent of disinfection by-products.
Grguric, Gordan. J. Chem. Educ. 2000, 77, 495.
Aqueous Solution Chemistry |
Equilibrium |
Kinetics |
Applications of Chemistry
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An Analogy to Help Students Understand Reaction Orders Charles J. Marzzacco
This article describes a simple analogy to help students understand the concept of the rate law for a chemical reaction. The analogy involves the mathematical relationships between various characteristics of a cube and the length of its edge.
Charles J. Marzzacco. J. Chem. Educ. 1998, 75, 482.
Learning Theories |
Kinetics |
Rate Law
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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
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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
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Interactive program system for integration of reaction rate equations Chesick, Jobn P.
93. The authors describe here a Pascal-language kinetics rate law integration package for the desktop microcomputer.
Chesick, Jobn P. J. Chem. Educ. 1988, 65, 599.
Rate Law |
Laboratory Computing / Interfacing |
Kinetic-Molecular Theory
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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
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Kinetics and mechanism-a games approach Harsch, Gunther
Using statistical games to simulate and illustrate a variety of chemical kinetics.
Harsch, Gunther J. Chem. Educ. 1984, 61, 1039.
Kinetics |
Mechanisms of Reactions |
Catalysis |
Rate Law
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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
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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
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The kinetics of running Larsen, Russell D.
The consideration of running as a rate process has several advantages for a student studying chemical kinetics for the first time.
Larsen, Russell D. J. Chem. Educ. 1979, 56, 651.
Kinetics |
Rate Law
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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
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Bimolecular nucleophilic displacement reactions Edwards, John O.
The bimolecular nucleophilic displacement reaction is important and should be included in any detailed discussion of kinetics and mechanism at an early undergraduate level.
Edwards, John O. J. Chem. Educ. 1968, 45, 386.
Reactions |
Nucleophilic Substitution |
Kinetics |
Mechanisms of Reactions
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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
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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
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Chemical dynamics for college freshmen Hammond, George S.; Gray, Harry B.
Suggestions for topics regarding chemical dynamics to be considered in freshman chemistry.
Hammond, George S.; Gray, Harry B. J. Chem. Educ. 1968, 45, 354.
Thermodynamics |
Kinetics |
Reactions |
Mechanisms of Reactions |
Rate Law
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Kinetics for the undergraduate: Introduction King, Edward L.
Introduces the ACS symposium entitled "Kinetics in the Undergraduate Curriculum."
King, Edward L. J. Chem. Educ. 1963, 40, 573.
Kinetics
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Method for determining order of a reaction Zimmerman, Howard K.
The method presented here is a substitution process that expresses various rate laws in terms of one initial concentration only.
Zimmerman, Howard K. J. Chem. Educ. 1963, 40, 356.
Kinetics
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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
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