Chemistry - Chemical Kinetics Question with Solution | TestHub

The given reaction is ${\mathrm{N}}_{2(\mathrm{g})}+3{\mathrm{H}}_{2(\mathrm{g})}⟶2{\mathrm{NH}}_{3(\mathrm{g})}$

The rate of reaction can be expressed as:

$-\frac{d[{\mathrm{N}}_2]}{dt}=-\frac{1}{3}\frac{d[{\mathrm{H}}_2]}{dt}=\frac{1}{2}\frac{d[{\mathrm{NH}}_3]}{dt}$

Given that the rate of formation of ${\mathrm{NH}}_3$ is $\frac{d[{\mathrm{NH}}_3]}{dt}=0.088\mathrm{mol}{\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$

The consumption rate of ${\mathrm{N}}_2$ is $-\frac{d[{\mathrm{N}}_2]}{dt}$

$-\frac{d[{\mathrm{N}}_2]}{dt}=\frac{1}{2}\times 0.088=0.044\mathrm{mol}{\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$

Answer: $0.044\mathrm{mol}{\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$