Question detail
If the concentration of products in a reversible reaction is decreased, how does this affect the equilibrium position (A-level cue 62300266 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 right to produce more products.
- B. The equilibrium will shift to the left to produce more reactants. (A-level cue 62300266 distractor 1)
- C. The equilibrium will remain unchanged. (A-level cue 62300266 distractor 2)
- D. The reaction will stop completely. (A-level cue 62300266 distractor 3)
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 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 62300266.
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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