The rate constant for a reaction at 40.0°C is exactly 3 times that at 20.0°C. Calculate the Arrhenius energy of activation for the reaction.

Explanation:

Relation between Arrhenius energy and rate constant is as follows.

The given data is as follows.

        = 3 times.

         R = 8.314 J/mol K

                 = 293 K

                  = 313 K

Now, putting the given values into the above formula as follows.

    1.098 =

                  = 41870 J/mol

Thus, we can conclude that Arrhenius energy of activation for the reaction is 41870 J/mol.

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