For the reaction, 2 N_2 O_5 → 4 NO_2+ O_2, the rate equation can be expressed in two ways -(d[ N_2 O_5])/(d t)=k[ N_2 O_5] and +(d[ NO_2])/(d t)=k^′[…

For the reaction, $\displaystyle 2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2$, the rate equation can be expressed in two $$\begin{aligned} & \text { ways }-\frac{d\left[\mathrm{~N}_2 \mathrm{O}_5\right]}{d t}=k\left[\mathrm{~N}_2 \mathrm{O}_5\right] \text { and } \\ & +\frac{d\left[\mathrm{NO}_2\right]}{d t}=k^{\prime}\left[\mathrm{N}_2 \mathrm{O}_5\right] \end{aligned} $$ k and $\displaystyle \mathrm{k}^{\prime}$ are related as :