For ${\mathrm{N}}_2{\mathrm{O}}_5\left( \right.$ in $\left.{\mathrm{CCl}}_4\right)\to 2{\mathrm{NO}}_2+\frac{1}{2}{\mathrm{O}}_2$, $\mathrm{K}=6\times {10}^{-4}{ \mathrm{s}}^{-1}$ at $350 \mathrm{K}$ and $\mathrm{K}=1.2\times {10}^{-3}{ \mathrm{s}}^{-1}$ at $360 \mathrm{K}$. Then, when temperature is changed to$380 \mathrm{K}$, value of $\mathrm{K}$ (in ${\mathrm{s}}^{-1}$ )

The given reaction is:

         ${\mathrm{N}}_2{\mathrm{O}}_5$ (in $\left.{\mathrm{CCl}}_4\right)\to 2{\mathrm{NO}}_2+\frac{1}{2}{\mathrm{O}}_2$,

Given the value of $\mathrm{K}$ at $350 \mathrm{K}$ is $\mathrm{K}=6\times {10}^{-4}{ \mathrm{s}}^{-1}$ and at $360 \mathrm{K}$ the value is $\mathrm{K}=1.2\times {10}^{-3}{ \mathrm{s}}^{-1}$.

As we know that on increasing the temperature of ${10}^{\mathrm{o}}\mathrm{C}$, the rate of reaction will be doubled.

So, at $370 \mathrm{K}$ the value of K will be $2.4\times {10}^{-3}{ \mathrm{s}}^{-1}$.

At $380 \mathrm{K}$ the value of K will be $4.8\times {10}^{-3}{ \mathrm{s}}^{-1}$.