Chemistry - Chemical Kinetics Question with Solution | TestHub

í52 × $6.8=h_{\mathrm{Hg}}\times 13.6$

$h_{\mathrm{Hg}}=\frac{152\times 6.8}{13.6}=76\mathrm{cm}$ (1 atm)

Initial pressure $=1\mathrm{atm}$

$\mathrm{A}(\mathrm{g})\rightleftharpoons 2\mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$

Initial pressure ${\mathrm{P}}_0=1\mathrm{atm}$

$\mathrm{t}=100$ min ${\mathrm{P}}_0-\mathrm{x}2\mathrm{x}\mathrm{x}$

Total pressure at $100\min ={\mathrm{P}}_0+2\mathrm{x}=1+1$

or, $2\mathrm{x}=1,\mathrm{x}=1/2$ or, ${\mathrm{k}}_{\mathrm{x}}=\frac{2.303}{100}\log \left(\frac{1}{1-\mathrm{x}}\right)$ $=\frac{2.303}{100}\times 0.3010=\frac{0.7}{100}=7\times 10^{-3}{\min }^{-1}$ $k_{\mathrm{r}}=\frac{k_{\mathrm{B}}}{2}\Rightarrow k_{\mathrm{B}}=14\times 10^{-3}{\min }^{-1}$

Half-life $=100\min ,t_{75\%}=2\times {\mathbf{t}}_{50\%}=200\min$ ${\mathbf{t}}_{87.5\%}=3\times {\mathbf{t}}_{50\%}=600\min$