A → B The rate constants of the above reaction at 200 K and 300 K are 0.03 min^-1 and 0.05 min^-1 respectively. The activation energy for the…

$\displaystyle A \rightarrow B$ The rate constants of the above reaction at $\displaystyle 200$ K and $\displaystyle 300$ K are $\displaystyle 0.03 \mathrm{~min}^{-1}$ and $\displaystyle 0.05 \mathrm{~min}^{-1}$ respectively. The activation energy for the reaction is $\displaystyle \_\_\_\_$J (Nearest integer) (Given : $\displaystyle \ln 10=2.3$ $$\begin{aligned} & \mathrm{R}=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \\ & \log 5=0.70 \\ & \log 3=0.48 \\ & \log 2=0.30) \end{aligned} $$