For the reaction A → B, the rate constant k (. in. s^-1) is given by log_10 k=20.35-((2.47 × 10^3))/T The energy of activation in kJ mol^-1 is \ \ \…

For the reaction $\displaystyle \mathrm{A} \rightarrow \mathrm{B}$, the rate constant $\displaystyle \mathrm{k}\left(\right.$ in $\displaystyle \left.\mathrm{s}^{-1}\right)$ is given by $$\log _{10} k=20.35-\frac{\left(2.47 \times 10^3\right)}{T} $$The energy of activation in $\displaystyle \mathrm{kJ} \mathrm{~mol}^{-1}$ is \_\_\_\_. (Nearest integer) [Given : $\displaystyle \mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ ]