Chemistry - Chemical Equilibrium Question with Solution | TestHub

${\mathrm{N}}_2{\mathrm{O}}_4$ decomposes partially as : ${\mathrm{N}}_2{\mathrm{O}}_4(\mathrm{g})\rightleftharpoons 2{\mathrm{NO}}_2(\mathrm{g})$. In an experiment, some ${\mathrm{N}}_2{\mathrm{O}}_4$ gas is taken in a vessel and heated to 300 K , at which equilibrium is established. At equilibrium pressure of 1.0 atm , the density of the equilibrium mixture is $\left(\frac{23}{9}\right)\mathrm{g}/\mathrm{L}$. Now, the gas is compressed slowly and isothermally till the density of new equilibrium mixture becomes $\left(\frac{23}{4.8}\right)\mathrm{g}/\mathrm{L}$. The new equilibrium pressure (in atm) is ( $\mathrm{R}=0.08\mathrm{L}-\mathrm{atm}/\mathrm{K}-\mathrm{mol}$ )