Calculate the activation energy of a reaction whose reaction rate at `300 K` double for `10 K` rise in temperature.

Explanation

To calculate the activation energy of a reaction whose rate doubles when the temperature increases from 300 K to 310 K, we can use the Arrhenius equation. Here’s the step-by-step solution:

### Step 1: Understand the relationship between rate constants and temperature
The problem states that the reaction rate doubles when the temperature increases by 10 K. This can be expressed mathematically as:
\[ \frac{R_2}{R_1} = \frac{K_2}{K_1} = 2 \]
where \( R_1 \) and \( R_2 \) are the reaction rates at temperatures \( T_1 \) and \( T_2 \) respectively.
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