The activation energy of a first order reaction at `300 K` is 60 `kJ mol^(-1)`. In the presence of a catalyst, the activation energy gets lowered to `50kJ mol^(-1)` at `300 K`. How many times the reaction rate change in the presence of a catalyst at the same temperature ?

Explanation

To solve the problem of how many times the reaction rate changes in the presence of a catalyst, we can use the Arrhenius equation and the relationship between the rate constants of the reaction with and without the catalyst.

### Step-by-Step Solution:

1. **Identify Given Data:**
- Activation energy without catalyst (Ea1) = 60 kJ/mol = 60000 J/mol
- Activation energy with catalyst (Ea2) = 50 kJ/mol = 50000 J/mol
- Temperature (T) = 300 K
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