The decomposition of $C{H}_3{N}_{2}C{H}_3,C{H}_3{N}_{2}C{H}_3(g)C_2{H}_6(g)+N_2(g)$ at $327C$ follows first order kinetics. Suppose we start with $0\mathrm{.}0745$mol of $C{H}_3{N}_{2}C{H}_3$ in a volume of $4\mathrm{.}9L.$ If it takes $3250s$ for the quantity of $C{H}_3{N}_{2}C{H}_3$ to drop to $0\mathrm{.}0231$mol, what is the half$-$life of this reaction at this temperature? A$.3\mathrm{.}60{10}^{-4}s$ B$.1\mathrm{.}92{10}^{3}s$ C$.2\mathrm{.}98s$ D$.1\mathrm{.}40{10}^{-5}s$ E$.4\mathrm{.}95{10}^{4}s$