F 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?

The value of activation barrier for the reaction is, 43.374 kJ/mol.

Explanation:

According to the Arrhenius equation,

or,

where,

= rate constant at = k

= rate constant at  = 3k

= activation energy for the reaction = ?

R = gas constant = 8.314 J/mol.K

= initial temperature =

= final temperature =

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

Therefore, the activation energy for the reaction is, 43.374 kJ/mol.

the correct answer would be d. hope this !