The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.275 M. What is the value of k for this reaction?
The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.275 M. What is the value of k for this reaction?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.275 M. What is the value of k for this reaction?
Expert Solution
Step 1
A ==> Products
Since it is 2nd order in A, we can write the rate equation as ...
Rate = k[A]2
The rate can be determined by the change in [A] with respect to time as ...
change in [A] = 0.740 M - 0.275 M = 0.465 M
change in time = 13.5 s
Rate = 0.465 M/13.5 s = 0.0344 M/s
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