Chemistry - Chemical Kinetics Question with Solution | TestHub

The rate of reaction $2{\mathrm{N}}_2{\mathrm{O}}_5⟶4{\mathrm{NO}}_2+{\mathrm{O}}_2$ can be written in three ways $\begin{array}{rl}\frac{-d\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]}{dt}& =k\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]\\ \frac{d\left[{\mathrm{NO}}_2\right]}{dt}& =k^{\prime }\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]\\ \frac{d\left[{\mathrm{O}}_2\right]}{dt}& =k^{\prime \prime }\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]\end{array}$ The relationship between $k$ and $k^{\prime }$ and between $k$ and $k^{\prime \prime }$ areNEET 2011 (Mains)