Chemistry - Chemical Kinetics Question with Solution | TestHub

$$\begin{array}{l}2{\mathrm{NO}}_2\underset{{\mathrm{k}}_2}{\stackrel{{\mathrm{k}}_1}{\rightleftharpoons }}{\mathrm{N}}_2{\mathrm{O}}_4\\ \text{ Rate }=-\frac{1}{2}\frac{\mathrm{d}\left[{\mathrm{NO}}_2\right]}{\mathrm{dt}}=k_1{\left[{\mathrm{NO}}_2\right]}^2-k_2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]\end{array}$$ $\therefore$ Rate of disappearance of ${\mathrm{NO}}_2$ i.e., $$-\frac{\mathrm{d}\left[{\mathrm{NO}}_2\right]}{\mathrm{dt}}=2k_1{\left[{\mathrm{NO}}_2\right]}^2-k_2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]$$