Question detail
Scenario ALC-a97b9fea: Which answer best applies Equilibrium constant Kc to the objective "Calculate Kc from equilibrium concentrations."?
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 evidence must be applied specifically to Equilibrium constant Kc using the ALC-a97b9fea context.
- B. A generic recall statement that does not use the ALC-a97b9fea context.
- C. A distractor that swaps Equilibrium constant Kc with a different A-Level Chemistry topic.
- D. A distractor that gives a conclusion without evidence for ALC-a97b9fea.
Answer
The evidence must be applied specifically to Equilibrium constant Kc using the ALC-a97b9fea context.
Explanation
The correct option is The evidence must be applied specifically to Equilibrium constant Kc using the ALC-a97b9fea context. It is unique to ALC-a97b9fea, names Equilibrium constant Kc, and links the answer to Calculate Kc from equilibrium concentrations.. Other options are weaker because they are generic, swap the topic, or make an unsupported conclusion.
Common mistake
Incorrect Kc Calculation
Students often forget to include the correct stoichiometric coefficients when constructing the Kc expression, leading to incorrect values.
To fix this, remember that the Kc expression is constructed using the concentrations of products raised to the power of their coefficients, divided by the concentrations of reactants raised to their coefficients. For example, for the reaction aA + bB ⇌ cC + dD, the Kc expression is Kc = [C]^c [D]^d / [A]^a [B]^b. Substitute the equilibrium concentrations into this formula, perform the calculations, and ensure you express the final answer with the correct units (mol/dm³).
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