Consider the following equilibrium, CO ( g )+2 H_2( g ) ⇌ CH_3 OH ( g ) 0.1 mol of CO along with a catalyst is present in a 2 dm^3 flask maintained…

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