The rate constant of a reaction is `1.5 xx 10^(7)s^(-1)` at `50^(@)`C and `4.5 xx 10^(7)s^(-1)` at `100^(@)`C. Calculate the value of activation energy for the reaction `(R=8.314 J K^(-1)mol^(-1))`

Explanation

To calculate the activation energy (Ea) for the reaction given the rate constants at two different temperatures, we can use the Arrhenius equation in the form of the logarithmic relationship:

\[ \log \left( \frac{k_2}{k_1} \right) = \frac{E_a}{2.303R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right) \]

### Step 1: Convert temperatures from Celsius to Kelvin
- Given temperatures:
...