Question detail
A reversible reaction at equilibrium has the following equation: A + B ⇌ C + D. If the concentration of A is increased, predict the effect on the position of equilibrium and explain your reasoning using Le Chatelier's Principle.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
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Topic
Reversible reactions and dynamic equilibrium
Question
A reversible reaction at equilibrium has the following equation: A + B ⇌ C + D. If the concentration of A is increased, predict the effect on the position of equilibrium and explain your reasoning using Le Chatelier's Principle.
Answer
Increasingthe concentration of A will shift the equilibrium to the right, towards the products cand D. This occurs because the system responds to oppose the change by consumingthe added reactant A.
Explanation
This answer demonstrates an understandingof Le chatelier's Principle and how changes in concentration affect equilibrium. It tests the ability to apply theoretical knowledge to predict the outcome of a specificchange in a chemical system. This answer is strongest when it stays anchored to The effect of changingconcentration (HT only) and directly addresses (HT only) Explain concentration effects usingLe chatelier's Principle.
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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