Chemistry - Chemical Kinetics Question with Solution | TestHub

Let the reaction be $$\begin{array}{rl}& \mathrm{A}\stackrel{k}{⟶}\text{ Product }\\ & \text{ Rate }=k[\mathrm{A}]\\ & 1.5\times 10^{-2}\mathrm{mol}{\text{L }}^{-1}{\min }^{-1}=\mathrm{k}[0.5]\\ & k=\frac{1.5\times 10^{-2}}{0.5}\\ & =3\times 10^{-2}{\min }^{-1}\\ & t_{1/2}=\frac{0.693}{k}\\ & \Rightarrow t_{1/2}=\frac{0.693}{3\times 10^{-2}}\\ & =0.231\times 10^2\min \\ & \Rightarrow t_{1/2}=23.1\min \end{array}$$ Related Theory Decay profiles for first-order reactions with large and small rate constants