Question

In the equilibrium reaction Ba(IO3)2 (s) ⇌ Ba^2+ + 2IO3^-, what is the equilibrium constant expression (Kc)?

a) Ba^2+IO3^-^2
b) Ba^2+/IO3^-
c) Ba^2+IO3^-
d) 1/Ba^2+IO3^-^2

Answer 1

The equilibrium constant expression for the reactions can be determined based on the concentrations of the reactants and products. If the concentration of products is greater than the concentration of reactants, the value of Kc will be greater than 1. If the concentration of reactants is greater, Kc will be less than 1. If the concentrations are roughly equal, Kc will be approximately 1.

Step-by-step explanation:

The equilibrium constant expression for the reaction represented by the equation AgCl(s) = Ag+ (aq) + Cl¯ (aq) is Kc = [Ag+][Cl¯] / [AgCl]. Whether Kc > 1, < 1, or ≈ 1 depends on the concentrations of the reactants and products. If the concentration of products is greater than the concentration of reactants, Kc will be greater than 1. If the concentration of reactants is greater than the concentration of products, Kc will be less than 1. If the concentrations are roughly equal, Kc will be approximately 1.

The equilibrium constant expression for the reaction represented by the equation Pb²+ ¯(aq) + 2Cl¯(aq) = PbCl₂ (s) is Kc = [PbCl₂] / [Pb²+][Cl¯]². Similar to the previous case, Kc depends on the concentrations of the reactants and products. The same principle applies, where if the concentration of products is greater than the concentration of reactants, Kc will be greater than 1. If the concentration of reactants is greater than the concentration of products, Kc will be less than 1. If the concentrations are roughly equal, Kc will be approximately 1.