Question detail
In a gaseous equilibrium, if the pressure is increased, what effect does this have if there are fewer moles of gas on the product side?
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 equilibrium will shift to the left.
- B. The equilibrium will shift to the right.
- C. The equilibrium will remain unchanged.
- D. The reaction will stop.
Answer
The equilibrium will shift to the right.
Explanation
The correct answer is The equilibrium will shift to the right.. This answer directly addresses the question: In a gaseous equilibrium, if the pressure is increased, what effect does this have if there are fewer moles of gas on the product side? 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 Temperature Effects
Students often think that increasing temperature always increases the rate of reaction rather than favoring the endothermic direction of a reversible reaction.
Focus on understanding that increasing temperature shifts equilibrium towards the endothermic direction, which may not always correlate with an increased 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.