Chemistry - Chemical Equilibrium Question with Solution | TestHub

The reaction is
${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{N}{\mathrm{O}}_2\left(\mathrm{g}\right)$
n = 2 and$\mathrm{\alpha }=\frac{20}{100}=0.2$
D = 4.6, initial vapour density
d = vapour density at equilibrium
$\mathrm{\alpha }=\frac{\mathrm{D}-\mathrm{d}}{(\mathrm{n}-1)\mathrm{d}}$
$0.2=\frac{46-\mathrm{d}}{(2-1)\mathrm{d}}$
d = 38.3
Molar mass equilibrium$=2\times 38.3=76.6$
$\text{PM}\text{=}\text{dRT}$
Here, d = density of gas mixture
$\text{d(mix)}\text{=}\frac{\text{PM}}{\text{RT}}\text{= }\frac{\text{1}\text{×}\text{76}\text{.6}}{\text{0}\text{.0821}\text{×}\text{300}}$
$\text{=}\text{3}\text{.12}\text{g/L}$