Chemistry - Chemical Equilibrium Question with Solution | TestHub

For the given reaction, $K=\frac{[\mathrm{HI}{]}^2}{\left[{\mathrm{H}}_2\right]\left[{\mathrm{I}}_2\right]}$ As 1 mole of ${\mathrm{H}}_2$ reacts with 1 mole of ${\mathrm{I}}_2$, even at equilibrium, $\left[{\mathrm{H}}_2\right]=\left[{\mathrm{I}}_2\right]$ Hence, $K=\frac{[\mathrm{HI}{]}^2}{{\left[{\mathrm{I}}_2\right]}^2}$ or $\sqrt{K}=\frac{[\mathrm{HI}]}{\left[{\mathrm{I}}_2\right]}=\sqrt{47.6}$ i.e., $[\mathrm{HI}]>\left[{\mathrm{I}}_2\right]$