How many kJ/mol must an enzyme lower the activation energy of the reaction to make it useful? We known that in the absence of a catalyst a certain biochemical reaction occurs x times per second at normal body temperature which is 37 degrees C. The reaction needs to occur 5000 times faster than when it's uncaralyzed in order to be physiological useful. For this problem use the Arrhenius expression for the rate constant k to derive the equation for deltaEa under constant temperature.
How many kJ/mol must an enzyme lower the activation energy of the reaction to make it useful? We known that in the absence of a catalyst a certain biochemical reaction occurs x times per second at normal body temperature which is 37 degrees C. The reaction needs to occur 5000 times faster than when it's uncaralyzed in order to be physiological useful. For this problem use the Arrhenius expression for the rate constant k to derive the equation for deltaEa under constant temperature.
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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How many kJ/mol must an enzyme lower the activation energy of the reaction to make it useful? We known that in the absence of a catalyst a certain biochemical reaction occurs x times per second at normal body temperature which is 37 degrees C. The reaction needs to occur 5000 times faster than when it's uncaralyzed in order to be physiological useful. For this problem use the Arrhenius expression for the rate constant k to derive the equation for deltaEa under constant temperature.
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