JEE Main 2025 Chemistry question
Consider the following equilibrium, CO(g) + 2H₂(g) CH₃OH(g) 0.1 mol of CO along with a catalyst is present in a 2 dm³ flask maintained at 500 K. Hydrogen is introduced into the flask until the pressure is 5 bar and 0.04 mol of CH₃OH is formed. The kp is × 10⁻³ (nearest integer). Given : R = 0.08 dm³ bar K⁻¹ mol⁻¹ Assume only methanol is formed as the product and the system follows ideal gas behaviour.
Answer: 74
Solution
= 5×2/(0.08×500) = 0.25. P(CH3OH)=0.8 bar, P(H2)=3 bar, P(CO)=1.2 bar. Kp = 0.8/(1.2×3²) = 0.07407 = 74.07×10⁻³.