Question detail
If the concentration of both reactants A and B is increased in the reaction A + B ⇌ C + D, what will be the effect on 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. Equilibrium shifts towards products
- B. Equilibrium shifts towards reactants
- C. No change in equilibrium position
- D. Equilibrium shifts randomly
Answer
The correct option is Equilibrium shifts towards products.
Explanation
The correct option is "Equilibrium shifts towards products" because it supports the approved learning objective: (HT only) Predict that increasing reactant concentration shifts equilibrium towards products. 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 Equilibrium Shifts
Students often think that increasing reactant concentration will shift the equilibrium towards reactants instead of products.
Remember that according to Le Chatelier's Principle, increasing the concentration of reactants will shift the equilibrium position towards the products to counteract the change.
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