Question detail
What is the consequence of shifting the equilibrium position to the right in a reaction with gaseous products?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Chemical equilibria, Le Chatelier's principle and Kc
Question
- A. Increased yield of products
- B. Decreased yield of products
- C. No change in yield
- D. Increased reaction time
Answer
Increased yield of products
Explanation
The correct option is Increased yield of products. Increased yield of products is the best answer because it directly supports the AQA A-Level Chemistry objective to use Le Chatelier's principle to predict the effect of pressure changes. This reasoning is anchored to Equilibrium and Le Chatelier's principle in Chemical equilibria, Le Chatelier's principle and Kc, and it separates Le Chatelier from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.
Common mistake
Pressure Change Misunderstanding
Students often think that increasing pressure will always shift the equilibrium to the right, regardless of the reaction.
To fix this, remember that increasing pressure shifts the equilibrium towards the side with fewer moles of gas. Always analyze the balanced equation to determine the effect of pressure changes.
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