Le Chatelier's Principle Applied to Haber Process Steps:

• Identify the reaction as exothermic (ΔH = -92 kJ/mol) and note fewer moles of gas on product side (4 → 2).
• Apply Le Chatelier's principle: increasing pressure shifts equilibrium to side with fewer gas moles, favoring NH₃ yield.
• For temperature, low temperature favors exothermic forward reaction, but kinetics limit rate.
• Evaluate each option's statement and reason for accuracy based on these principles. Why A is correct:
• It correctly states high pressure increases yield, reasoned by Le Chatelier's principle favoring fewer moles, matching the 4:2 gas ratio. Why the others are wrong:
• B: Claims high temperature increases yield; incorrect, as exothermic reaction favors low temperature per Le Chatelier.
• C: Says catalyst increases yield; wrong, as catalysts speed equilibrium attainment but don't shift position.
• D: Asserts low pressure favors products; false, as more moles on reactant side means low pressure favors reactants.

Final answer: A