Question detail
What happens to the rate of the forward and reverse reactions as a reversible reaction approaches equilibrium?
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. The forward reaction rate decreases while the reverse increases
- B. Both rates increase indefinitely
- C. Both rates become equal
- D. The forward reaction stops
Answer
Both rates become equal
Explanation
The correct answer is Both rates become equal. This answer directly addresses the question: What happens to the rate of the forward and reverse reactions as a reversible reaction approaches equilibrium? 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 Closed Systems
Students often think that equilibrium means the reaction has stopped, rather than understanding that reactions continue at the same rate in a closed system.
Emphasize that at equilibrium, both the forward and reverse reactions are still occurring, but their rates are equal, maintaining constant concentrations of reactants and products.
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