Equilibrium Constant and Reaction Quotient
This worksheet covers the concepts of equilibrium constant (Kc and Kp) and reaction quotient (Qc and Qp), including calculations and their application in predicting reaction direction.
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Equilibrium Constant and Reaction Quotient
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Read each question carefully and provide your answers in the space provided. Show all your work for calculation problems.
1. Which of the following statements is true regarding the equilibrium constant (Kc)?
It changes with changes in reactant or product concentrations.
It is affected by the presence of a catalyst.
It is a constant value for a given reaction at a specific temperature.
Its value depends on the initial amounts of reactants.
2. For the reaction A(g) + 2B(g) ⇌ C(g), if Qc > Kc, which statement is true?
The reaction will proceed to the right to reach equilibrium.
The reaction will proceed to the left to reach equilibrium.
The reaction is already at equilibrium.
The value of Kc will increase to match Qc.
1. The equilibrium constant (Kc) is a ratio of concentrations to concentrations, each raised to the power of their stoichiometric coefficients.
2. When a system is at equilibrium, the rate of the forward reaction is to the rate of the reverse reaction.
3. The reaction quotient (Qc) can be calculated at point in a reaction, while Kc is only applicable at .
1. Write the expression for the equilibrium constant (Kc) for the following reaction:
2SO2(g) + O2(g) ⇌ 2SO3(g)
2. Explain the difference between Kc and Kp. When is it appropriate to use each?
1. Consider the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g). At a certain temperature, an equilibrium mixture contains 0.20 M N2, 0.30 M H2, and 0.50 M NH3. Calculate the value of Kc for this reaction at this temperature.
2. For the reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g), Kc = 1.3 x 10^-2 at 1000 K. If at a specific moment, the concentrations are [NO] = 0.10 M, [Br2] = 0.05 M, and [NOBr] = 0.02 M, in which direction will the reaction proceed to reach equilibrium? Justify your answer.
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