According to Le Chatelier's principle, how does increasing total pressure at constant temperature affect the Haber equilibrium: N2(g) + 3 H2(g) <=> 2 NH3(g)?
Answer and explanation
Correct answer: C. It shifts the equilibrium toward the right
- Step 1: The reactants have 1 + 3 = 4 moles of gas, while products have 2 moles of gas. Step 2. Increasing pressure shifts equilibrium toward the side with fewer gas moles (forward direction), increasing NH3 yield. Answer: It shifts the equilibrium toward the right. Why not the others: Equilibrium constant K_p is altered only by temperature changes, not pressure changes.
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