N_2 O_5(g) → 2 NO_2(g)+1/2 O_2(g) In the above first order reaction the initial concentration of N_2 O_5 is 2.40 × 10^-2 mol L^-1 at 318 K. The…

$$\mathrm{N}_2 \mathrm{O}_{5(g)} \rightarrow 2 \mathrm{NO}_{2(g)}+\frac{1}{2} \mathrm{O}_{2(g)} $$ In the above first order reaction the initial concentration of $\displaystyle \mathrm{N}_2 \mathrm{O}_5$ is $\displaystyle 2.40 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$ at $\displaystyle 318$ K . The concentration of $\displaystyle \mathrm{N}_2 \mathrm{O}_5$ after $\displaystyle 1$ hour was $\displaystyle 1.60 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$. The rate constant of the reaction at $\displaystyle 318$ K is \_\_\_\_ $\displaystyle \times 10^{-3} \mathrm{~min}^{-1}$. (Nearest integer) [Given : $\displaystyle \log 3=0.477, \log 5=0.699$ ]