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?

Answer : The activation energy for the reaction is, 52.9 kJ/mol

Explanation :

According to the Arrhenius equation,

or,

where,

= initial temperature =

= final temperature =

= rate constant at =

= rate constant at =

= activation energy for the reaction = ?

R = gas constant = 8.314 J/mole.K

Now put all the given values in this formula, we get:

Therefore, the activation energy for the reaction is, 52.9 kJ/mol

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