2CO(g) + O₂(g) ⇌ 2CO₂(g). High pressure will favour the forward reaction because the process

Correct answer: the process occurs with a decrease in volume.

Explanation: By Le Châtelier’s principle, increasing pressure shifts equilibrium toward the side with fewer moles of gas. Here, the forward reaction goes from 3 moles of gas (2 CO + 1 O₂) to 2 moles of gas (2 CO₂), i.e., a decrease in volume. Hence high pressure favours the forward reaction.

• High pressure favours gas formation – Incorrect; it favours the side with fewer gas moles, not gas formation per se.
• The reaction is in dynamic equilibrium – True but irrelevant to the pressure effect.
• The reaction is exothermic – Temperature, not pressure, is the key for exothermic/endothermic shifts.