Le Chatelier's Principle Application to Methanol Synthesis

Steps:

• Identify stoichiometry: 3 moles gas (left) vs. 1 mole gas (right), so pressure increase favors products.
• Note ΔH negative: exothermic, so temperature increase favors reactants.
• Given pressure 4 × 10^3 Pa (low, ~0.04 atm) and 150°C (moderate): low pressure disfavors products; high temperature disfavors products.
• Evaluate statements: correct ones address equilibrium shift correctly under these conditions.

Why D is correct:

• D accurately states low pressure and high temperature both shift equilibrium left, per Le Chatelier's principle for mole decrease and exothermic reactions.

Why the others are wrong:

• A: Wrong; increasing pressure shifts right, but given pressure is too low to favor yield significantly.
• B: Wrong; reaction is exothermic (ΔH < 0), so temperature rise shifts left, not right.
• C: Wrong; no catalyst mentioned, and conditions alone don't guarantee high yield without one.

Final answer: D