For the exothermic Haber process reaction: N2(g) + 3 H2(g) <=> 2 NH3(g) (Delta H = -92 kJ/mol), how will increasing the total pressure at constant temperature affect the equilibrium position?
Answer and explanation
Correct answer: D. Shifts equilibrium to the right, producing more NH3
By Le Chatelier's principle, increasing pressure favors the side with fewer moles of gas. The reactant side has 1 + 3 = 4 moles of gas, while product side has 2 moles of gas. Thus, equilibrium shifts right to favor NH3 formation.
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