Practice Scenario 1: Calculating The Value Of K From Equilibrium Concentrations/partial Pressures (6.3.1)

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6 sample questions

Question 1.
What does the equilibrium constant (K) represent?
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Think about what you measure in a reversible reaction.
Question 2.
Is Kc calculated using concentrations or pressures?
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Recall the Kc formula.
3Question 3.
What does Kc represent in a chemical reaction?
- Ratio of reactants only
- Ratio of products only
- Ratio of products to reactants at equilibrium
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Focus on the definition of Kc.
4Question 4.
True or False: The value of Kc is temperature independent.
- True
- False
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Think of how temperature affects reactions.
Question 5.
In a reaction where 2A = B + C, if Kc = 4 at a specific temperature, determine the equilibrium concentrations if the initial concentration of A is 2.0 M in a closed system.
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Be careful with coefficients in your calculations!
Question 6.
If Kp = 0.050 for the reaction A + 2B ⇌ C, what change in conditions will favor the production of C? Explain why.
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Consider the mole count on each side of the equation!

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