The rate constant for the order reaction increases from `4 xx 10^(-2)` to `24 xx 10^(-2)` when the temperature changes from 300K to 350 K. Calculate energy of activation for this reaction.

Explanation

To calculate the energy of activation (Ea) for the reaction, we can use the Arrhenius equation in its logarithmic form. The equation relates the rate constants (k1 and k2) at two different temperatures (T1 and T2) to the activation energy.

### Step-by-Step Solution:

1. **Identify the given values:**
- \( k_1 = 4 \times 10^{-2} \, \text{s}^{-1} \) at \( T_1 = 300 \, K \)
- \( k_2 = 24 \times 10^{-2} \, \text{s}^{-1} \) at \( T_2 = 350 \, K \)
- Universal gas constant \( R = 8.314 \, \text{J/(mol K)} \)
...