Question detail
What happens to the equilibrium position when the concentration of a reactant is decreased in a reversible reaction (A-level cue 44ba4994 focus)
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 left to produce more reactants.
- B. The equilibrium will shift to the right to produce more products. (A-level cue 44ba4994 distractor 1)
- C. The equilibrium will remain unchanged. (A-level cue 44ba4994 distractor 2)
- D. The reaction will stop completely. (A-level cue 44ba4994 distractor 3)
Answer
The equilibrium will shift to the left to produce more reactants.
Explanation
The correct option is The equilibrium will shift to the left to produce more reactants.. The equilibrium will shift to the left to produce more reactants. is correct because it supports the objective: Use Le Chatelier's principle to predict the effect of concentration changes.. The reasoning stays within Equilibrium and Le Chatelier's principle and avoids drifting into a similar A-Level Chemistry idea. This version is uniquely anchored to Equilibrium and Le Chatelier's principle. Retrieval anchor: A-level cue 44ba4994.
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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