The initial concentration of ${\mathrm{N}}_2{\mathrm{O}}_5$ in the following first order reaction:

${\mathrm{N}}_2{{\mathrm{O}}_5}_{\left(\mathrm{g}\right)}\to 2{\mathrm{NO}}_{2\left(\mathrm{g}\right)}+\frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}$ was $1.24\times {10}^{-2} \mathrm{mol}/\mathrm{L}$ at 318 K. The concentration of ${\mathrm{N}}_2{\mathrm{O}}_5$ after 60 minutes was $0.20\times {10}^{-2} \mathrm{mol}/\mathrm{L}$. The rate constant of the reaction in ${\min }^{-1}$ is  $\mathrm{x}\times {10}^{-2}$, value of x is $\left[\log 6.2=0.792\right]$.