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Chapter 15: Problem 82

Silver chloride, \(\mathrm{AgCl}(s)\), is an insoluble strong electrolyte. (a) Write the equation for the dissolution of \(\mathrm{AgCl}(s)\) in \(\mathrm{H}_{2} \mathrm{O}(l)\) (b) Write the expression for \(K_{c}\) for the reaction in part (a). (c) Based on the thermochemical data in Appendix \(\mathrm{C}\) and Le Ch芒telier's principle, predict whether the solubility of \(\mathrm{AgCl}\) in \(\mathrm{H}_{2} \mathrm{O}\) increases or decreases with increasing temperature.

Short Answer

Expert verified
(a) The dissolution equation for AgCl in water is: \[\text{AgCl(s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^鈭� (aq) \] (b) The expression for Kc is: \[K_c = [\text{Ag}^+][\text{Cl}^-]\] (c) The dissolution of AgCl in water is an endothermic reaction (螖H > 0). According to Le Ch芒telier's principle, increasing the temperature will increase the solubility of AgCl in water.

Step by step solution

01

Part (a): Dissolution Equation

Silver chloride is an insoluble strong electrolyte. When it dissolves in water, it dissociates into its respective ions. The dissolution equation for AgCl can be represented as follows: \[ \text{AgCl(s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^鈭� (aq) \]
02

Part (b): Expression for Kc

The equilibrium constant, Kc, can be determined by expressing the concentration of products divided by the concentration of reactants. In our case, since AgCl is a solid, it is not included in the Kc expression. So, the expression for Kc can be written as follows: \[K_c = [\text{Ag}^+][\text{Cl}^-]\]
03

Part (c): Solubility and Temperature

According to Le Ch芒telier's principle, if we increase the temperature of an endothermic reaction, the equilibrium will shift towards the products side, increasing the solubility. In contrast, if we increase the temperature of an exothermic reaction, the equilibrium will shift towards the reactants side, decreasing the solubility. We need to find out whether the dissolution of AgCl in water is an endothermic or exothermic reaction by referring to the thermochemical data provided in Appendix C. Based on the data, we find that the dissolution of AgCl in water has a positive enthalpy change (螖H > 0), which indicates that it is an endothermic reaction. Therefore, according to Le Ch芒telier's principle, increasing the temperature will shift the equilibrium towards the products side and increase the solubility of AgCl in water.

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Most popular questions from this chapter

Methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) can be made by the reaction of \(\mathrm{CO}\) with \(\mathrm{H}_{2}\) : $$ \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g) $$ (a) Use thermochemical data in Appendix \(C\) to calculate \(\Delta H^{\circ}\) for this reaction. (b) To maximize the equilibrium yield of methanol, would you use a high or low temperature? (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?

Suppose that the gas-phase reactions \(\mathrm{A} \longrightarrow \mathrm{B}\) and \(\mathrm{B} \longrightarrow \mathrm{A}\) are both elementary processes with rate con- stants of \(3.8 \times 10^{-2} \mathrm{~s}^{-1}\) and \(3.1 \times 10^{-1} \mathrm{~s}^{-1}\), respectively. (a) What is the value of the equilibrium constant for the equilibrium \(\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g) ?\) (b) Which is greater at equilibrium, the partial pressure of A or the partial pressure of B? Explain.

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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The equilibrium \(2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{NOCl}(g)\) is established at \(500 \mathrm{~K}\). An equilibrium mixture of the three gases has partial pressures of \(0.095 \mathrm{~atm}, 0.171 \mathrm{~atm}\), and \(0.28\) atm for \(\mathrm{NO}, \mathrm{Cl}_{2}\), and \(\mathrm{NOCl}\), respectively. Calculate \(K_{p}\) for this reaction at \(500 \mathrm{~K}\).
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