${N_2}{O_{5(g)}} \to 2N{O_{2(g)}} + {1 \over 2}{O_{2(g)}}$
In the above first order reaction the initial concentration of N₂O₅ is 2.40 $\times$ 10^$-$2 mol L^$-$1 at 318 K. The concentration of N₂O₅ after 1 hour was 1.60 $\times$ 10^$-$2 mol L^$-$1. The rate constant of the reaction at 318 K is ______________ $\times$ 10^$-$3 min^$-$1. (Nearest integer)
[Given : log 3 = 0.477, log 5 = 0.699]