Question detail
In a system at equilibrium, what is the effect of increasing pressure if the reaction has equal numbers of gaseous molecules on both sides?
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 shifts to the right
- B. The equilibrium shifts to the left
- C. No effect on the equilibrium position
- D. The reaction rate increases
Answer
No effect on the equilibrium position
Explanation
The correct answer is No effect on the equilibrium position. This answer directly addresses the question: In a system at equilibrium, what is the effect of increasing pressure if the reaction has equal numbers of gaseous molecules on both sides? 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 believe that changing pressure will always affect the equilibrium position, regardless of the number of gas molecules on each side.
Remember that pressure changes only affect equilibrium position when there is a difference in the number of gas molecules on each side of the equation.
Related flashcards
Flashcard 1 of 6
Related practice questions
Question 1 of 5
Choose an answer, get feedback, then move sideways through the set.