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Chapter 15: Problem 35

(a) How does a reaction quotient differ from an equilibrium constant? (b) If \(Q_{c}

Short Answer

Expert verified
(a) The reaction quotient (Qc) represents the ratio of product concentrations to reactant concentrations at any particular moment during a reaction, while the equilibrium constant (Kc) represents this ratio when the reaction has reached equilibrium, with no further changes in concentration. (b) If \(Q_c < K_c\), the reaction will proceed in the forward direction to reach equilibrium, converting more reactants into products. (c) For \(Q_c\) to be equal to \(K_c\), the reaction must be at equilibrium, with no further changes in concentrations of reactants and products.

Step by step solution

01

(a) Differences Between Reaction Quotient and Equilibrium Constant

The reaction quotient (Qc) and equilibrium constant (Kc) both represent the ratio of product concentrations to reactant concentrations for a chemical reaction. However, Qc represents this ratio at any particular moment during the reaction's progress, while Kc represents this ratio when the reaction has reached equilibrium, and the concentrations of products and reactants no longer change with time.
02

(b) Determining Reaction Direction based on Qc and Kc values

To determine the direction of a reaction, we need to compare the values of Qc and Kc: - If \(Q_c < K_c\), it means that the concentration of the products is lower than what would be expected at equilibrium. To reach equilibrium, the reaction needs to proceed in the forward direction, converting more reactants into products. - If \(Q_c > K_c\), it means that the concentration of products is higher than what would be expected at equilibrium. To reach equilibrium, the reaction needs to proceed in the reverse direction, converting more products back into reactants. In this case, as \(Q_c < K_c\), the reaction will proceed in the forward direction to reach equilibrium.
03

(c) Condition for Qc to be equal to Kc

For the reaction quotient (Qc) to be equal to the equilibrium constant (Kc), the reaction must be at equilibrium. It means that the concentrations of the reactants and products have stopped changing with time and are in a balanced state.

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Most popular questions from this chapter

Write the expression for \(K_{c}\) for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. (a) \(3 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{NO}_{2}(g)\) (b) \(\mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons \mathrm{CS}_{2}(g)+4 \mathrm{H}_{2}(g)\) (c) \(\mathrm{Ni}(\mathrm{CO})_{4}(g) \rightleftharpoons \mathrm{Ni}(s)+4 \mathrm{CO}(g)\) (d) \(\mathrm{HF}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{F}^{-}(a q)\) (e) \(2 \mathrm{Ag}(s)+\mathrm{Zn}^{2+}(a q) \rightleftharpoons 2 \mathrm{Ag}^{+}(a q)+\mathrm{Zn}(s)\)

The reaction \(\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g)\) has \(K_{p}=0.0870\) at \(300^{\circ} \mathrm{C}\). A flask is charged with \(0.50\) atm \(\mathrm{PCl}_{3}, 0.50 \mathrm{~atm} \mathrm{Cl}_{2}\), and \(0.20 \mathrm{~atm} \mathrm{PCl}_{5}\) at this tempera- ture. (a) Use the reaction quotient to determine the direction the reaction must proceed to reach equilibrium. (b) Calculate the equilibrium partial pressures of the gases. (c) What effect will increasing the volume of the system have on the mole fraction of \(\mathrm{C}_{2}\) in the equilibrium mixture? (d) The reaction is exothermic. What effect will increasing the temperature of the system have on the mole fraction of \(\mathrm{Cl}_{2}\) in the equilibrium mixture?

A mixture of \(\mathrm{H}_{2} \mathrm{~S}\), and \(\mathrm{H}_{2} \mathrm{~S}\) is held in a 1.0-L vessel at \(90^{\circ} \mathrm{C}\) until the following equilibrium is achieved: $$ \mathrm{H}_{2}(g)+\mathrm{S}(s) \rightleftharpoons \mathrm{H}_{2} \mathrm{~S}(g) $$ At equilibrium the mixture contains \(0.46 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{~S}\) and \(0.40 \mathrm{~g} \mathrm{H}_{2}\). (a) Write the equilibrium- constant expression for this reaction. (b) What is the value of \(K_{c}\) for the reaction at this temperature? (c) Why can we ignore the amount of \(S\) when doing the calculation in part \((b)\) ?

(a) At \(1285{ }^{\circ} \mathrm{C}\) the equilibrium constant for the reaction \(\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{Br}(g)\) is \(K_{c}=1.04 \times 10^{-3} .\) A \(0.200-\mathrm{L}\) vessel containing an equilibrium mixture of the gases has \(0.245 \mathrm{~g}\) \(\mathrm{Br}_{2}(g)\) in it. What is the mass of \(\mathrm{Br}(g)\) in the vessel? (b)For the reaction \(\mathrm{H}_{2}(g)+\mathrm{l}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g), K_{c}=55.3\) at \(700 \mathrm{~K}\). In a 2.00-L flask containing an equilibrium mixture of the three gases, there are \(0.056 \mathrm{~g} \mathrm{H}_{2}\) and \(4.36 \mathrm{~g} \mathrm{I}_{2}\). What is the mass of HI in the flask?

At \(2000^{\circ} \mathrm{C}\) the equilibrium constant for the reaction $$ 2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) $$ is \(K_{c}=2.4 \times 10^{3}\). If the initial concentration of \(\mathrm{NO}\) is \(0.200 \mathrm{M}\), what are the equilibrium concentrations of NO, \(\mathrm{N}_{2}\), and \(\mathrm{O}_{2} ?\)
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