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Kinetics : ArrheniusActEnergy (4 Variations)
The rate constant for the first-order dehydration of tert-butyl alcohol at 500oC is 1.20 x 10 -4 s -1. The rate constant for this process at 600oC is 6.80 x 10 -3 s -1. Calculate the activation energy for this reaction in kJ/mol. (R = 8.314 J/mol K)
Kinetics |
Chemometrics
Kinetics : ArrheniusTemp (3 Variations)
The activation energy for the isomerization of cyclopropane to propene is 274 kJ/mol. By what factor does the rate of reaction increase as the temperature rises from 500oC to 550oC assuming all else remains constant? (R = 8.314 J/mol k)
Hint: This is asking for the ratio of rates which is proportional to the ratio of the rate constants, all else being equal.
(1) Based on the units of the rate constant, what is the order of the reaction? {1:MULTICHOICE:zero-order#No, that is not correct.~=first-order#Correct!~second-order#No, that is not correct.~third-order#No, that is not correct.}
(2) What is the concentration of CH3CN after 0.20 minutes of reaction if the initial concentration is 0.10 M? {1:NUMERICAL:=4e-4:1e-5#Correct!~%50%4e-4:5e-5#Close, but not quite.}(Do not include units!)
Data Pooling in a Chemical Kinetics Experiment: The Aquation of a Series of Cobalt(III) ComplexesRichard 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
An Experimental Approach to Teaching and Learning Elementary Statistical MechanicsFrank 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
Visualizing the Transition State: A Hands-on Approach to the Arrhenius EquationThomas 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.
ChemPaths 104 M Feb 21John W. Moore Today in Chem 104:
* Lecture: Rate Laws
* Reading:
Kotz:, Ch. 15, Sec. 3-4
Moore, Ch. 13, Sec. 3-5
* Homework #5 due by 11:55 pm F Feb 25
* Excel assignment due in first discussion section this week
* Quiz 4 in second discussoin section
Kinetics |
Rate Law
The Rate EquationEd Vitz, John W. Moore A section of ChemPrime, the Chemical Educations Digital Library's free General Chemistry textbook.
Kinetics |
Rate Law
Unimolecular ProcessesEd Vitz, John W. Moore A section of ChemPrime, the Chemical Educations Digital Library's free General Chemistry textbook.
