Question detail
If the concentration of reactants is decreased in a reversible reaction, what will happen to the equilibrium position?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Reversible reactions and dynamic equilibrium
Question
- A. It will shift towards the reactants
- B. It will shift towards the products
- C. It will remain unchanged
- D. It will shift to the left
Answer
The correct option is It will shift towards the reactants.
Explanation
The correct option is "It will shift towards the reactants" because it supports the approved learning objective: (HT only) Explain concentration effects using Le Chatelier's Principle. The other options are incorrect or weaker because they are vague, use the wrong Chemistry context, or do not clearly explain the answer for The effect of changing concentration (HT only).
Common mistake
Misunderstanding Le Chatelier's Principle
Students often think that changing the concentration of reactants or products will always shift the equilibrium towards the side with fewer molecules, without considering the specific reaction conditions.
To fix this, students should remember that Le Chatelier's Principle states that a system at equilibrium will shift to oppose the change. They should analyze the specific reaction and the number of moles on each side to predict the direction of the shift accurately.
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