Question

the first order reaction is formed to have K= 5.5 ? 10^-14 s^-1.find half life of the reaction

Answer 1

Dear Student,

$$\begin{gathered} \mathrm{For}\mathrm{the}\mathrm{first}\mathrm{order}\mathrm{reaction}, \\ {\mathrm{t}}_{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.}=\frac{0.693}{\mathrm{k}} \\ \mathrm{Here},\mathrm{k}=5.5\times {10}^{-14}{\mathrm{s}}^{-1} \\ \mathrm{Therefore},{\mathrm{t}}_{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.}=\frac{0.693}{5.5\times {10}^{-14}{\mathrm{s}}^{-1}}=0.126\times {10}^{14}\mathrm{s}{}^{\mathrm{or}}12.6\times {10}^{12}\mathrm{s} \end{gathered}$$