If a temperature increase from 18.0 ∘C to 37.0 ∘C triples the rate constant for a reaction, what is the value of the activation barrier for the reaction?

Answer : The activation energy for the reaction is, 43.4 KJ

Explanation :

According to the Arrhenius equation,

or,

where,

= rate constant at

= rate constant at =

= activation energy for the reaction = ?

R = gas constant = 8.314 J/mole.K

= initial temperature =

= final temperature =

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

Therefore, the activation energy for the reaction is, 43.4 KJ

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