Consider the following equilibrium,
$\mathrm{CO}(\mathrm{~g})+2 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_3 \mathrm{OH}(\mathrm{~g})$
0.1 mol of CO along with a catalyst is present in a $2d{m^3}$ flask maintained at 500 K . Hydrogen is introduced into the flask until the pressure is 5 bar and 0.04 mol of $C{H_3}OH$ is formed. The $K_p^\theta $ is ______ $ \times {10^{ - 3}}$ (nearest integer).
Given : $R = 0.08d{m^3}$ bar ${K^{ - 1}}mo{l^{ - 1}}$
Assume only methanol is formed as the product and the system follows ideal gas behaviour.