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d. Since k1 is equal to 3.8 x 109 s-1, k-1 is equal to 9.8 x 10^8M-1s-1 and k2 is equal to 2.3 x 10^6M-1s-1, and that the activation energy for the overall process was determined to be 135.2 kJ mol-1 when measured at 300 K, calculate the overall k value for the reaction at T= 550 K.

d. Since k1 is equal to 3.8 x 109 s-1, k-1 is equal to 9.8 x 10^8M-1s-1 and k2 is equal to 2.3 x 10^6M-1s-1, and that the activation energy for the overall process was determined to be 135.2 kJ mol-1 when measured at 300 K, calculate the overall k value for the reaction at T= 550 K.

Chemistry
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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They told me to repost PLEASE JUST THE LAST QUESTION PART D
For the following basic steps, A2 = A + A (fast; k1, k-1) A + B ---> Products (k2) a. What is the molecularity of the direct step 2 process? b. Using the pre-equilibrium approximation, derive the expression for the predicted rate law for product formation. vs. What is the overall order of the reaction? d. Since k1 is equal to 3.8 x 109 s-1, k-1 is equal to 9.8 x 10^8M-1s-1 and k2 is equal to 2.3 x 10^6M-1s-1, and that the activation energy for the overall process was determined to be 135.2 kJ mol-1 when measured at 300 K, calculate the overall k value for the reaction at T = 550 K.
Transcribed Image Text:For the following basic steps, A2 = A + A (fast; k1, k-1) A + B ---> Products (k2) a. What is the molecularity of the direct step 2 process? b. Using the pre-equilibrium approximation, derive the expression for the predicted rate law for product formation. vs. What is the overall order of the reaction? d. Since k1 is equal to 3.8 x 109 s-1, k-1 is equal to 9.8 x 10^8M-1s-1 and k2 is equal to 2.3 x 10^6M-1s-1, and that the activation energy for the overall process was determined to be 135.2 kJ mol-1 when measured at 300 K, calculate the overall k value for the reaction at T = 550 K.
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