The activation energy for the decomposition of hydrogen peroxide is 42 kJ/mol, 2H₂O₂(aq)-> 2H₂O₂(1) + O₂(g) whereas when the reaction is catalyzed by the enzyme catalase, it is 7.0 kJ/mol. Calculate the temperature that would cause the uncatalyzed reaction to proceed as rapidly as the enzyme-catalyzed decomposition at 25°C. Assume the frequency factor A to be the same in both cases.

The activation energy for the decomposition of hydrogen peroxide is 42 kJ/mol, 2H₂O₂(aq)-> 2H₂O₂(1) + O₂(g) whereas when the reaction is catalyzed by the enzyme catalase, it is 7.0 kJ/mol. Calculate the temperature that would cause the uncatalyzed reaction to proceed as rapidly as the enzyme-catalyzed decomposition at 25°C. Assume the frequency factor A to be the same in both cases.

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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