Final answer:
The equilibrium expression for the dissociation reaction AgCl(s) = Ag+ (aq) + Cl− (aq) is Kc = [Ag+][Cl-]. Pure solids and liquids are not included in the equilibrium constant expression.
Step-by-step explanation:
The equilibrium expression for a reaction relates the concentrations of products to the concentrations of reactants at equilibrium. To write an equilibrium expression, one would use the concentrations of the products raised to their stoichiometric coefficients over the concentrations of the reactants raised to their stoichiometric coefficients.
For the specific chemical reaction provided, AgCl(s) = Ag+ (aq) + Cl− (aq), which is a dissociation reaction, the correct equilibrium constant expression (Kc) would be Kc = [Ag+][Cl−]. Recall that pure solids and liquids are not included in the equilibrium expression. The concentration of AgCl is not included in the expression because it is a solid and its concentration is constant. Regarding the magnitude of Kc, we can infer that it is less than 1, because the solubility of AgCl is low, thus yielding low concentrations of both Ag+ and Cl− ions at equilibrium.