Consider the following reaction: A+B→C+DA+B→C+D The initial concentrations of the reactants AA and BB are 0.260 M� and 0.400 M�, respectively. The rate of reaction is 0.060 M⋅s−1�⋅s−1, and the orders of the reaction, with respect to reactants AA and BB, are 1 and 2, respectively. Determine the rate constant (k�) for the reaction using the rate law.
Consider the following reaction: A+B→C+DA+B→C+D The initial concentrations of the reactants AA and BB are 0.260 M� and 0.400 M�, respectively. The rate of reaction is 0.060 M⋅s−1�⋅s−1, and the orders of the reaction, with respect to reactants AA and BB, are 1 and 2, respectively. Determine the rate constant (k�) for the reaction using the rate law.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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Consider the following reaction:
A+B→C+DA+B→C+D
The initial concentrations of the reactants AA and BB are 0.260 M� and 0.400 M�, respectively.
The rate of reaction is 0.060 M⋅s−1�⋅s−1, and the orders of the reaction, with respect to reactants AA and BB, are 1 and 2, respectively.
Determine the rate constant (k�) for the reaction using the rate law.
Express your answer in M−2⋅s−1�−2⋅s−1 to three significant figures.
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