Question detail
If the concentration of reactants is increased 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 products.
- B. It will shift towards the reactants.
- C. It will remain unchanged.
- D. It will shift to the left.
Answer
It will shift towards the products.
Explanation
The correct answer is It will shift towards the products.. This answer directly addresses the question: If the concentration of reactants is increased in a reversible reaction, what will happen to the equilibrium position? It matches the approved Chemistry 8462 learning objective and the linked subtopic. The other options are incorrect because they either change the rate, catalyst, reversible reaction, equilibrium, or graph context, or they do not answer the exact point being tested.
Common mistake
Misunderstanding Product Concentration Effects
Students often predict that increasing product concentration shifts equilibrium towards products instead of reactants.
Remember that increasing product concentration actually shifts the equilibrium towards the reactants, as per Le Chatelier's Principle.
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