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 prevent the escape of heat.
- B. To ensure no reactants or products are lost.
- C. To maintain constant temperature.
- D. To allow for continuous reaction.
Answer
To ensure no reactants or products are lost.
Explanation
The correct answer is To ensure no reactants or products are lost.. 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 Le Chatelier's Principle
Students often state that a system at equilibrium will always shift to the side with more products when a change is imposed.
Remember that Le Chatelier's Principle states that a system at equilibrium responds to oppose the change, which may mean shifting towards reactants or products depending on the specific change.
Related flashcards
Flashcard 1 of 5
Related practice questions
Question 1 of 5
Choose an answer, get feedback, then move sideways through the set.