Chemistry - Chemical Kinetics Question with Solution | TestHub

For the given reaction:

${\mathrm{NO}}_{2(\mathrm{g})}+{\mathrm{CO}}_{(\mathrm{g})}\to {\mathrm{NO}}_{(\mathrm{g})}+{\mathrm{CO}}_{2(\mathrm{g})}$

The rate of reaction is given by:

$\text{Rate}=-\frac{d[{\mathrm{NO}}_2]}{dt}=-\frac{d[\mathrm{CO}]}{dt}=+\frac{d[\mathrm{NO}]}{dt}=+\frac{d[{\mathrm{CO}}_2]}{dt}$

Given that the rate of formation of ${\mathrm{NO}}_{(\mathrm{g})}$ is:

$+\frac{d[\mathrm{NO}]}{dt}=\mathrm{Y}{\text{ mol dm}}^{-3}{\text{ s}}^{-1}$

The rate of disappearance of ${\mathrm{CO}}_{(\mathrm{g})}$ is $-\frac{d[\mathrm{CO}]}{dt}$.

From the rate equation:

$-\frac{d[\mathrm{CO}]}{dt}=+\frac{d[\mathrm{NO}]}{dt}=\mathrm{Y}{\text{ mol dm}}^{-3}{\text{ s}}^{-1}$

Thus, the rate of disappearance of ${\mathrm{CO}}_{(\mathrm{g})}$ is $\mathrm{Y}{\text{ mol dm}}^{-3}{\text{ s}}^{-1}$.

Answer: $\mathrm{Y}\mathrm{mol}{\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$