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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 80QRT: When enzymes are present at very low concentration, their effect on reaction rate can be described...

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