Chemistry - Chemical Kinetics Question with Solution | TestHub

$$\begin{array}{rl}\text{ Rate of reaction }& =-\frac{1}{2}\frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=-\frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}=\frac{1}{3}\frac{\mathrm{d}[\mathrm{C}]}{\mathrm{dt}}\\ \text{ Rate of reaction }& =\frac{1}{3}\frac{\mathrm{d}[\mathrm{C}]}{\mathrm{dt}}\\ & =\frac{1}{3}\times 1.3\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\\ & =0.433\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\end{array}$$ $\therefore$ Rate of disappearance of $\mathrm{A}$ $$\begin{array}{rl}& =2\times 0.433\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\\ & =0.866\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\\ & =8.66\times 10^{-5}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\end{array}$$