9.2 g of ${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)$ is taken in a closed 1 L vessel and heated till the following equilibrium is reached<br> ${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)\leftrightharpoons2{\rm{N}}{{\rm{O}}_2}\left( {\rm{g}} \right)$<br> At equilibrium, 50% ${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)$ is dissociated. What is the equilibrium constant $\left( {{\rm{in}}\;{\rm{ mol}}{{\rm{L}}^{ - 1}}} \right)$? (Molecular weight of ${{\rm{N}}_2}{{\rm{O}}