Chemistry - Chemical Kinetics Question with Solution | TestHub

For a zero-order reaction:

$${\mathrm{Cl}}_2{\mathrm{O}}_7(\mathrm{g})⟶2{\mathrm{ClO}}_2(\mathrm{g})+\frac{3}{2}{\mathrm{O}}_2(\mathrm{g})$$

Rate of reaction = $-\frac{d[{\mathrm{Cl}}_2{\mathrm{O}}_7]}{dt}=50mmHg$

Rate of production of ${\mathrm{O}}_2=\frac{3}{2}\times 50=75mmHg$

Half-life, $t_{1/2}=\frac{P_o}{2k}=\frac{600}{2\times 50}=6sec$

Therefore, rate of production of ${\mathrm{O}}_2$ and half-life period are $75mmHg$ and $6sec$ respectively.