Question detail
If a reaction at equilibrium is subjected to an increase in pressure, which of the following statements is true?
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 reaction will always favor the formation of products.
- B. The equilibrium will shift towards the side with fewer gas molecules.
- C. The equilibrium will shift towards the side with more gas molecules.
- D. The reaction will stop completely.
Answer
The equilibrium will shift towards the side with fewer gas molecules.
Explanation
The correct answer is The equilibrium will shift towards the side with fewer gas molecules.. This answer directly addresses the question: If a reaction at equilibrium is subjected to an increase in pressure, which of the following statements is true? 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 Pressure Effects
Students often think that increasing pressure will always increase the rate of reaction rather than shifting the equilibrium position.
Remember that increasing pressure shifts the equilibrium towards the side with fewer gas molecules, which may not necessarily increase the reaction rate.
Related flashcards
Flashcard 1 of 5
Related practice questions
Question 1 of 5
Choose an answer, get feedback, then move sideways through the set.