Chemistry - Chemical Kinetics Question with Solution | TestHub

${\mathrm{O}}_3\stackrel{\text{ Fast }}{⟶}{\mathrm{O}}_2+\mathrm{O}$ $$\begin{array}{l}\mathrm{O}+{\mathrm{O}}_3\stackrel{\text{ Slow }}{⟶}2{\mathrm{O}}_2\\ \mathrm{k}=\frac{\left[{\mathrm{O}}_2\right][\mathrm{O}]}{\left[{\mathrm{O}}_3\right]}\\ \text{ Rate }={\mathrm{k}}^{\prime }\left[{\mathrm{O}}_3\right][\mathrm{O}]\end{array}$$ put [O] from (ii) $$\mathrm{r}=\frac{{\mathrm{k}}^{\prime }\left[{\mathrm{O}}_3\right]\mathrm{k}\left[{\mathrm{O}}_3\right]}{\left[{\mathrm{O}}_2\right]}=\mathrm{k}{\left[{\mathrm{O}}_3\right]}^2{\left[{\mathrm{O}}_2\right]}^{-1}$$ Note: Intermediates are never represented in rate law equation.