JEE Main 2025 — 2 April, Morning Shift — Question 20

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 $2 \mathrm{dm}^{3}$ flask maintained at 500 K . Hydrogen is introduced into

the flask until the pressure is 5 bar and 0.04 mol of $\mathrm{CH}_{3} \mathrm{OH}$ is formed. The $\mathrm{K}_{\mathrm{p}}^{\theta}$ is $\_\_\_\_\_$ $10^{-3}$ (nearest

integer). Given : $\mathrm{R}=0.08 \mathrm{dm}^{3}$ bar $\mathrm{K}^{-1} \mathrm{~mol}^{-1}$ Assume only methanol is formed as the product and the

system follows ideal gas behaviour.