Chemistry - Chemical Kinetics Question with Solution | TestHub

For the reaction $2{\text{N}}_2{\text{O}}_5\to 4{\text{NO}}_2+{\text{O}}_2$, the rate of reaction is given by:

$\text{Rate}=\frac{1}{4}\frac{d[{\text{NO}}_2]}{dt}$

Given that the rate of formation of ${\text{NO}}_2$ is $\frac{d[{\text{NO}}_2]}{dt}=0.025{\text{ mol L}}^{-1}{\text{s}}^{-1}$.

Substituting the value:

$\text{Rate}=\frac{1}{4}\times 0.025$

$\text{Rate}=0.00625{\text{ mol L}}^{-1}{\text{s}}^{-1}$

$\text{Rate}=6.25\times 10^{-3}{\text{ mol L}}^{-1}{\text{s}}^{-1}$

Answer: $6.25\times 10^{-3}mol{L}^{-1}{S}^{-1}$