The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at 300 K is 1.0 × 10^-3 s^-1 and the activation…

The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at $\displaystyle 300$ K is $\displaystyle 1.0 \times 10^{-3} \mathrm{~s}^{-1}$ and the activation energy $\displaystyle \mathrm{E}_{\mathrm{a}}=11.488 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the rate constant at $\displaystyle 200$ K is \_\_\_\_ $\displaystyle \times 10^{-5} \mathrm{~s}^{-1}$. (Round off to the Nearest Integer). (Given : $\displaystyle \mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )