Le Chatelier's Principle in Haber Process

Steps:

• Identify the ammonia synthesis reaction: N₂ + 3H₂ ⇌ 2NH₃ (Δn = -2, fewer moles on product side).
• Apply Le Chatelier's principle: increasing pressure shifts equilibrium toward the side with fewer gas moles to counteract the change.
• Note that 200 atm is high pressure, favoring ammonia yield despite the reaction's exothermic nature.
• Conclude that high pressure is essential for industrial viability, but equilibrium yield alone isn't the full story.

Why D is correct:

• High pressure overcomes the low equilibrium constant at typical temperatures, enabling economic production rates per the industrial Haber-Bosch process.

Why the others are wrong:

• A: Incorrectly focuses only on equilibrium yield; high pressure also addresses kinetics and catalyst efficiency, not just yield.
• B: Not enough information.
• C: Not enough information.

Final answer: D