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\( \mathrm{N}_{2} \mathrm{O}_{5}(\mathrm{~g}) \rightarrow 2 \mathrm{NO}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \). In the above first order reaction the initial concentration of \( \mathrm{N}_{2} \mathrm{O}_{5} \), is \( 2.40 \times 10^{-2} \mathrm{~mol} \) \( \mathrm{L}^{-1} \) at \( 318 \mathrm{~K} \). The concentration of \( \mathrm{N}_{2} \mathrm{O}_{5} \), after 1 hour was \( 1.60 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \). The rate constant of the reaction at 318 \( \mathrm{K} \) is \( \times 10^{-3} \mathrm{~min}^{-1} \). (Nearest integer) [Given: \( \log 3= \) \( 0.47 \overline{\log 5}=0.699] \)
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