Question detail
Which statement best explains why concentrations remain constant at dynamic 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. At dynamic equilibrium, the forward and reverse reaction rates are equal, so reactant and product concentrations stay constant.
- B. The forward reaction has stopped, so no more products are made.
- C. Only the reverse reaction continues, so product concentration steadily falls.
- D. Reactants and products have identical concentrations at equilibrium.
Answer
The correct option is At dynamic equilibrium, the forward and reverse reaction rates are equal, so reactant and product concentrations stay constant.
Explanation
The correct option is "At dynamic equilibrium, the forward and reverse reaction rates are equal, so reactant and product concentrations stay constant." because equilibrium is dynamic: both reactions continue at the same rate. The other options are wrong because equilibrium does not mean reactions stop, does not mean only the reverse reaction continues, and does not require equal reactant and product concentrations.
Common mistake
Misunderstanding Equilibrium Concentrations
Students often think that the concentrations of reactants and products are equal at equilibrium.
Emphasize that at equilibrium, the concentrations remain constant but are not necessarily equal.
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