For the reaction, K_p is — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

0.1 mole of CH₃OH is formed, consuming 0.1 mole of CO and 0.2 mole of H₂. At equilibrium: n(CH₃OH) = 0.1 mol, n(CO) = 0.20 - 0.1 = 0.1 mol. Let the equilibrium moles of H₂ be x. Total moles n_total = 0.1 + 0.1 + x = 0.2 + x. Using PV = nRT: 7.5 × 2.463 = (0.2 + x) × 0.0821 × 750 => 18.4725 = (0.2 + x) × 61.575 => 0.2 + x = 0.3 => x = 0.1 mol. Equilibrium partial pressures: P_CO = (0.1/0.3) × 7.5 = 2.5 atm, P_H₂ = (0.1/0.3) × 7.5 = 2.5 atm, P_CH₃OH = (0.1/0.3) × 7.5 = 2.5 atm. K_p = P_CH₃OH / (P_CO × P_H₂²) = 2.5 / (2.5 × 2.5²) = 1 / 6.25 = 0.16 atm⁻². Therefore, correct answer is A.