Chemistry - Chemical Kinetics Question with Solution | TestHub

For the reaction, $2{\mathrm{NH}}_3\to {\mathrm{N}}_2+3{\mathrm{H}}_2$

From equation (i) and (ii)
$\therefore$ Rate of production of ${\mathrm{N}}_2,\frac{d\left[{\mathrm{N}}_2\right]}{dt}=k$ $=2.5\times 10^{-4}\mathrm{mol}\mathrm{L}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$ From equation (iii) Rate of production of ${\mathrm{H}}_2,\frac{d\left[{\mathrm{H}}_2\right]}{dt}=3k$ $\begin{array}{rl}& =3\times 2.5\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\\ & =7.5\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}\end{array}$