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 using the given rate constants at two different temperatures, we will use the Arrhenius equation in the logarithmic form:

\[ \log\left(\frac{K_2}{K_1}\right) = \frac{E_a}{2.303R}\left(\frac{1}{T_1} - \frac{1}{T_2}\right) \]

### Step-by-Step Solution:

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