For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) at equilibrium, which change will shift the equilibrium to the right (toward products)?
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Correct answer
D. Decreasing the volume of the container
Principle or equation
Le Chatelier's principle: for a gaseous equilibrium, decreasing volume increases pressure, shifting equilibrium toward the side with fewer moles of gas. Here, product side has 2 moles, reactant side has 4 moles, so shift right.
Why this answer is correct
Increasing volume decreases pressure, shifting toward more moles (left). Decreasing N2 shifts left. Increasing NH3 shifts left. Decreasing volume increases pressure, shifting toward fewer moles, which is the product side (2 mol vs 4 mol), so equilibrium shifts right.
Example
For 2A(g) ⇌ B(g), decreasing volume shifts right because product side has fewer moles.
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