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Journal Articles: 47 results
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
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
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 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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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
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 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
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
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
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
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