AIIMS 2018 Chemistry Le Chatelier's Principle MCQ Question

Increasing pressure at constant temperature favors the solubility of gases in liquids due to Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract changes. Since gas molecules occupy more volume, increasing pressure shifts the equilibrium towards the dissolved state, enhancing solubility. In contrast, option A is incorrect because the Haber process (N₂(g) + 3H₂(g) ⇌ 2NH₃(g)) is favored by high pressure, making the rate increase, not decrease. Option C is incorrect as the solubility of solids in liquids is generally unaffected by pressure, and option D is incorrect because the reaction 2C(s) + CO₂(g) → 2CO(g) would shift left, favoring the formation of solid carbon (C) under increased pressure.