Question detail
If the Kc value for a reaction is 10^3, what does this imply about the equilibrium position?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Chemical equilibria, Le Chatelier's principle and Kc
Question
- A. The equilibrium position favors the products significantly.
- B. The equilibrium position favors the reactants significantly.
- C. The reaction is at equilibrium with no preference.
- D. The reaction will not reach equilibrium.
Answer
The equilibrium position favors the products significantly.
Explanation
The correct option is The equilibrium position favors the products significantly.. The equilibrium position favors the products significantly. is the best answer because it directly supports the AQA A-Level Chemistry objective to interpret the magnitude of Kc in terms of equilibrium position. This reasoning is anchored to Equilibrium constant Kc in Chemical equilibria, Le Chatelier's principle and Kc, and it separates magnitude of Kc from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.
Common mistake
Misunderstanding Kc Values
Students often confuse the magnitude of Kc with the direction of the reaction's favorability, believing that a larger Kc always indicates a reaction that goes to completion.
To correct this, students should understand that a large Kc value indicates that at equilibrium, the concentration of products is much greater than that of reactants, but it does not mean the reaction goes to completion.
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