At `25^(@)C` the activation energy for a catalysed reaction is `126 KJ mol^(-1)` and for uncatalysed reaction is `350 KJ mol^(-1)` . How many times the rates is increased in the presence of catalyst ?

Explanation

To solve the problem of how many times the rates of a reaction are increased in the presence of a catalyst, we can use the Arrhenius equation, which relates the rate constants of reactions to their activation energies. The formula we will use is:

\[ \frac{k_1}{k_2} = e^{\left(\frac{E_a^{uncatalyzed} - E_a^{catalyzed}}{RT}\right)} \]

Where:
- \( k_1 \) is the rate constant of the catalyzed reaction.
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