Chemistry - Chemical Kinetics Question with Solution | TestHub

For first order reaction $A⟶B$ Given that rate $=k\times [A]$ Rate $=2.0\times 10^{-5}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$ $[A]=$ Conc. of $A=0.01\mathrm{M}$ So, $2.0\times 10^{-5}=k\times 0.01$ $\begin{array}{rl}k& =\frac{2.0\times 10^{-5}}{0.01}{\mathrm{s}}^{-1}\\ & =2.0\times 10^{-3}{\mathrm{s}}^{-1}\end{array}$ For first order reaction $\begin{array}{rl}{T}_{1/2}& =\frac{0.693}{k}=\frac{0.693}{2.0\times 10^{-3}}\\ & =346.5\approx 347\mathrm{s}\end{array}$