The activation energy of one of the reactions in a biochemical process is 532611 J mol^-1. When the temperature falls from 310 K to 300 K, the change…

The activation energy of one of the reactions in a biochemical process is $\displaystyle 532611 \mathrm{~J} \mathrm{~mol}^{-1}$. When the temperature falls from $\displaystyle 310$ K to $\displaystyle 300$ K, the change in rate constant observed is $\displaystyle \mathrm{k}_{300}=x \times 10^{-3} \mathrm{k}_{310}$. The value of $\displaystyle x$ is \_\_\_\_. [Given : $$\begin{aligned} & \ln 10=2.3 \\ & \left.\mathrm{R}=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right] \end{aligned} $$