Question detail
In a reversible reaction at equilibrium, if the concentration of reactants is increased, what will happen to the position of equilibrium?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Chemical equilibria, Le Chatelier's principle and Kc
Question
- A. The equilibrium will shift to the right to produce more products.
- B. The equilibrium will shift to the left to produce more reactants.
- C. The equilibrium will remain unchanged.
- D. The reaction will stop completely.
Answer
The equilibrium will shift to the right to produce more products.
Explanation
The correct option is The equilibrium will shift to the right to produce more products.. The equilibrium will shift to the right to produce more products. is the best answer because it directly supports the AQA A-Level Chemistry objective to use Le Chatelier's principle to predict the effect of concentration changes. This reasoning is anchored to Equilibrium and Le Chatelier's principle in Chemical equilibria, Le Chatelier's principle and Kc, and it separates Le Chatelier from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.
Common mistake
Misunderstanding Concentration Changes
Students often believe that increasing the concentration of reactants will always lead to a shift in equilibrium towards the products without considering the system's response.
To fix this, remember that according to Le Chatelier's principle, increasing the concentration of reactants causes the system to shift towards the products to counteract the change. This shift results in an increase in product formation until a new equilibrium is established, which may not always be significant if the reaction is already product-favored.
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