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Journal Articles: 42 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
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
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
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
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
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
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
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
KineticsLab: The Crystal Violet/Sodium Hydroxide Reaction  Cannon, John F.; Gammon, Steven D.; Hunsberger, Lynn R.
A computer-assisted experiment to collect and analyze data for a kinetic study of the decolorization of crystal violet in basic solution.
Cannon, John F.; Gammon, Steven D.; Hunsberger, Lynn R. J. Chem. Educ. 1994, 71, 238.
Kinetics |
Rate Law |
Reactions
The activation energy of a slap bracelet   Kramer, F. Axtell.
This accessory/toy can be used to help students understand activation energy.
Kramer, F. Axtell. J. Chem. Educ. 1993, 70, 1002.
Kinetics |
Reactions |
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
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
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
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
Enthalpy and Hot Wheels: An analogy  Bonneau, Marcia C.
Demonstrating the relationship between activation energy and the heat of a reaction using a "Hot Wheels" track and car to simulate a potential energy diagram.
Bonneau, Marcia C. J. Chem. Educ. 1987, 64, 486.
Kinetics |
Calorimetry / Thermochemistry |
Thermodynamics
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
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
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
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
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.
212-215. Four questions requiring applications of chemistry and their solutions.
Campbell, J. A. J. Chem. Educ. 1975, 52, 727.
Rate Law |
Nuclear / Radiochemistry
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
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
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 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
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
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
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
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
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
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