Question detail

When the concentration of products is increased in a reversible reaction, what is the expected effect on the equilibrium position (A-level cue 07d84414 focus)

Try the question, check the answer, then read the explanation to understand the curriculum point.

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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 07d84414 distractor 1)
C. The equilibrium will remain unchanged. (A-level cue 07d84414 distractor 2)
D. The reaction will stop completely. (A-level cue 07d84414 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 07d84414.

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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