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

The equation $\mathrm{k}=\left(6.5\times {10}^{12}{ \mathrm{s}}^{-1}\right){\mathrm{e}}^{-26000 \mathrm{K}/\mathrm{T}}$ is followed for the decomposition of compound $\mathrm{A}$. The activation energy for the reaction is ____ $\mathrm{KJ} {\mathrm{mol}}^{-1}$. [nearest integer]

(Given: $\mathrm{R}=8.314 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)

For the decomposition of azomethane. ${\mathrm{CH}}_3{ \mathrm{N}}_2{\mathrm{CH}}_3\left(\mathrm{g}\right)\to {\mathrm{CH}}_3{\mathrm{CH}}_3\left(\mathrm{g}\right)+{\mathrm{N}}_2$ a first order reaction, the variation in partial pressure with time at $600 \mathrm{K}$ is given as

The half life of the reaction is____$\times {10}^{-5} \mathrm{s}$

$2\mathrm{NO}+2{\mathrm{H}}_2\to {\mathrm{N}}_2+2{\mathrm{H}}_2\mathrm{O}$

The above reaction has been studied at $800 °\mathrm{C}$. The related data are given in the table below

The order of the reaction with respect to NO is____

$\begin{array}{ccc}\left[\mathrm{A}\right]& \to & \left[\mathrm{B}\right]\\ \mathrm{Reactant}& & \mathrm{Product}\end{array}$

If formation of compound $\left[\mathrm{B}\right]$ follows the first order of kinetics and after $70$ minutes the concentration of $\left[\mathrm{A}\right]$ was found to be half of its initial concentration. Then the rate constant of the reaction is $\mathrm{x}\times {10}^{-6}{ \mathrm{s}}^{-1}$. The value of $\mathrm{x}$ is____