Question detail
A reversible reaction at equilibrium has the following balanced equation: A(g) + B(g) ⇌ C(g) + D(g). If the concentration of A 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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Topic
Reversible reactions and dynamic equilibrium
Question
A reversible reaction at equilibrium has the following balanced equation: A(g) + B(g) ⇌ C(g) + D(g). If the concentration of A is increased, predict the effect on the position of equilibrium and explain your reasoning using Le Chatelier's Principle.
Answer
Increasingthe concentration of A will shift the equilibrium to the right, towards the products cand D. This occurs because the system opposes the change by consumingthe added reactant A.
Explanation
This question tests the understandingof Le chatelier's Principle and how changes in concentration affect equilibrium. The answer demonstrates knowledge of the principle and its application to predict the direction of the shift. 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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