For the gaseous equilibrium N2(g) + 3 H2(g) <=> 2 NH3(g) (ΔH < 0), which perturbation will shift the equilibrium position to the right (favoring ammonia production)?

Answer and explanation

Correct answer: C. Decreasing the total system volume (increasing pressure)

According to Le Chatelier's principle, decreasing system volume increases total pressure, which causes the system to shift toward the side with fewer moles of gas. The reactants have 1 + 3 = 4 moles of gas, while the products have 2 moles of gas; thus the equilibrium shifts to the right. Because the reaction is exothermic, increasing temperature shifts it to the left.

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