One mole of a compound, AB  reacts with one mole of a compound CD according to the equation :
$AB\left(g\right)+CD\left(g\right)\rightleftharpoons AD\left(g\right)+CB\left(g\right)$ ; when equilibrium had been established it was found that $\frac{3}{4}$ mole each of reactants AB and CD had been converted to AD and CB. There is no change in volume. The equilibrium constant for the reaction is

Density of equilibrium mixture of ${\mathrm{N}}_2{\mathrm{O}}_4$ and ${\mathrm{NO}}_2$ at $1 \mathrm{atm}$ and $384 \mathrm{K}$ is $1.84\mathrm{g}/{\mathrm{dm}}^3$. Equilibrium constant of the following reaction is:
${\mathrm{N}}_2{\mathrm{O}}_4\rightleftharpoons 2{\mathrm{NO}}_2$

Assertion : Adding inert gas to dissociation equilibrium of ${\mathrm{N}}_2{\mathrm{O}}_4$ at constant temperature and pressure increases the dissociation.

Reason : Due to the addition of inert gas molar concentration of reactants and products decreases.

$2\mathrm{ICl}⟶{\mathrm{l}}_2+{\mathrm{Cl}}_2 {\mathrm{K}}_{\mathrm{C}}=0.14$

Initial concentration of $\mathrm{ICl}$ is $0.6\mathrm{M}$

Then equilibrium concentration of ${\mathrm{I}}_2$ is: