Question detail
Why is a closed system required when applying equilibrium predictions?
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. To allow for gas exchange with the environment.
- B. To prevent changes in temperature.
- C. To ensure that no reactants or products escape the system.
- D. To maintain constant pressure.
Answer
To ensure that no reactants or products escape the system.
Explanation
The correct answer is To ensure that no reactants or products escape the system.. This answer directly addresses the question: Why is a closed system required when applying equilibrium predictions? 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 always increases the rate of reaction instead of understanding that it affects the position of equilibrium.
Focus on how increasing pressure shifts equilibrium towards the side with fewer gas molecules, as explained by Le Chatelier's Principle.
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