Answered step by step
Verified Expert Solution
Question
1 Approved Answer
The activation energy for the decomposition of hydrogen peroxide is 42kJ/mol, 2H2O2(aq)2H2O2(l)+O2(g) whereas when the reaction is catalyzed by the enzyme catalase, it is 7.0kJ/mol.
The activation energy for the decomposition of hydrogen peroxide is 42kJ/mol, 2H2O2(aq)2H2O2(l)+O2(g) whereas when the reaction is catalyzed by the enzyme catalase, it is 7.0kJ/mol. Calculate the temperature that would cause the uncatalyzed reaction to proceed as rapidly as the enzyme-catalyzed decomposition at 25C. Assume the frequency factor A to be the same in both cases. The answer is _ 103K (answer format: _._)
Step by Step Solution
There are 3 Steps involved in it
Step: 1
Get Instant Access to Expert-Tailored Solutions
See step-by-step solutions with expert insights and AI powered tools for academic success
Step: 2
Step: 3
Ace Your Homework with AI
Get the answers you need in no time with our AI-driven, step-by-step assistance
Get Started