Question detail
In a closed system, the equilibrium of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is established. If the pressure is increased, predict the effect on the position of equilibrium and explain your reasoning using Le Chatelier's Principle.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
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exam_style
Style
Topic
Reversible reactions and dynamic equilibrium
Question
In a closed system, the equilibrium of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is established. If the pressure is increased, predict the effect on the position of equilibrium and explain your reasoning using Le Chatelier's Principle.
Answer
Increasingthe pressure will shift the equilibrium to the right, towards the production of NH3. This is because there are fewer moles of gas on the product side (2 moles of NH3) compared to the reactant side (4 moles of N2 and H2 combined).
Explanation
This question assesses the ability to apply Le chatelier's Principle to predict the effect of pressure changes on equilibrium. The answer shows understandingof how the number of gas moles influences the equilibrium position. This answer is strongest when it stays anchored to The effect of changingconditions on equilibrium (HT only) and directly addresses (HT only) Explain that changingconcentration, temperature or pressure can change the position of equilibrium.
Common mistake
Misinterpreting Le Chatelier’s Principle
Students often think that changing a condition simply speeds up the reaction, not that it shifts the equilibrium position.
Explain that Le Chatelier’s Principle predicts a shift in the position of equilibrium to oppose the change, not a change in the overall reaction rate. Clarify that the system moves to restore the original balance of reactants and products, not just to react faster.
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