According to Le Chatelier's Principle, how does increasing total pressure affect the equilibrium position of N2(g) + 3H2(g) <=> 2NH3(g)?
Answer and explanation
Correct answer: A. Shifts the equilibrium toward the forward direction
- Step 1: Increasing pressure shifts equilibrium toward the side with fewer moles of gas to relieve the pressure increase. Step 2. Gaseous reactants have 4 moles, while products have 2 moles. The system shifts forward to produce more ammonia. Answer: Shifts the equilibrium toward the forward direction (more NH3 produced). Why not the others: Backward shift would occur if products had more moles; no effect occurs when Delta n = 0; reactions never stop at equilibrium.
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