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