The rate of a reaction increases four times when the temperature changes from 300K to 320 K. Calculate the energy of activation of the reaction. `(R=8.314JK^(-1)mol^(-1))`

Explanation

To solve the problem of calculating the energy of activation (Ea) for a reaction where the rate increases four times when the temperature changes from 300 K to 320 K, we can use the Arrhenius equation in its logarithmic form.

### Step-by-Step Solution:

1. **Understand the Problem**: We know that the rate of a reaction increases by a factor of 4 when the temperature changes from 300 K to 320 K. We need to find the activation energy (Ea) using the Arrhenius equation.

2. **Use the Arrhenius Equation**: The Arrhenius equation can be expressed in logarithmic form as:
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