Chemistry - Chemical Kinetics Question with Solution | TestHub

For the given reaction $2{\text{N}}_2{\text{O}}_{5(g)}\to 4{\text{NO}}_{2(g)}+{\text{O}}_{2(g)}$

The rate of reaction is given by:

$\text{Rate}=-\frac{1}{2}\frac{d[{\text{N}}_2{\text{O}}_5]}{dt}=\frac{1}{4}\frac{d[{\text{NO}}_2]}{dt}=\frac{d[{\text{O}}_2]}{dt}$

Given the rate of disappearance of ${\text{N}}_2{\text{O}}_5$ is $-\frac{d[{\text{N}}_2{\text{O}}_5]}{dt}=0.06{\text{ mol dm}}^{-3}{\text{ s}}^{-1}$

The rate of formation of ${\text{O}}_2$ is:

$\frac{d[{\text{O}}_2]}{dt}=\frac{1}{2}\left(-\frac{d[{\text{N}}_2{\text{O}}_5]}{dt}\right)$

$\frac{d[{\text{O}}_2]}{dt}=\frac{1}{2}\times 0.06=0.03{\text{ mol dm}}^{-3}{\text{ s}}^{-1}$