Chemistry - Chemical Kinetics Question with Solution | TestHub

$$\begin{array}{rl}& \text{ rate of reaction }=2\times 10^{-5}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\\ & \Rightarrow \text{ order of reaction is }n=1\\ & \text{ rate }=\mathrm{K}[\mathrm{A}{]}^n\\ & [\mathrm{A}]=0.01\mathrm{M}\\ & \Rightarrow \mathrm{K}=\frac{2\times 10^{-5}}{0.01}=2\times 10^{-3}\\ & \mathrm{K}=\frac{0.693}{t_{1/2}}\\ & t_{1/2}=\frac{0.693}{2\times 10^{-3}}=346.5\mathrm{s}\end{array}$$ Related Theory For a first-order reaction, a graph plotted with $\ln [A]$ on the $Y$-axis and time on the $X$-axis, will be a straight line with a slope of $-k$.