Practice Equilibrium Constant In Gaseous Systems (6.4.1)

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6 sample questions

Question 1.
Define Kc.
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Remember, it’s a ratio of products to reactants.
Question 2.
Explain Le Chatelier's Principle in your own words.
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Think about how a system tries to maintain balance.
3Question 3.
Kc for a reaction is 10^3. If at equilibrium, reactants' concentration is higher than products, what direction does the reaction favor?
- Forward
- Reverse
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Consider what 'favors' means in this context.
4Question 4.
True or False? The equilibrium constant K changes with temperature.
- True
- False
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Think about factors that affect chemical reactions.
Question 5.
Given a reaction at equilibrium with Kc = 2.0 and initial concentrations of A = 1.0 M, and B = 1.0 M, how can you find the equilibrium concentrations of A and B?
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Keep in mind the stoichiometry of the reaction.
Question 6.
For the reaction 2NO(g) + O2(g) ⇌ 2NO2(g), given initial concentrations and an equilibrium constant of 58.4, how would you find the amount of NO2 formed?
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Use an ICE table to organize your data.

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