Chemistry, 20.02.2020 22:01 bartlettcs9817
Reaction is found to have a rate constant of 12.5 s-1 at 25.0 Celsius. When you heat the reaction up by ten degrees Celsius, the rate of the reaction exactly doubles. What is the activation energy for this reaction in kJ/mol?
Answers: 2
![\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]](/tpl/images/0517/9661/6d953.png)
= initial temperature = 
= final temperature = 
= rate constant at 
= 
= rate constant at 
= 
= activation energy for the reaction = ?![\log (\frac{25.0s^{-1}}{12.5s^{-1}})=\frac{Ea}{2.303\times 8.314J/mole.K}[\frac{1}{298.0K}-\frac{1}{308.0K}]](/tpl/images/0517/9661/6e305.png)
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Reaction is found to have a rate constant of 12.5 s-1 at 25.0 Celsius. When you heat the reaction up...
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