Question

In a generic reaction A+B ->C+D, 1.00 mol of A and 1.00 mol of B are allowed to react in a 1-L flask until equilibrium is established. If the equilibrium concentration of A is 0.450 mol/L, what is the equilibrium concentration of each of the other substances? What is Keq?

Answer 1

To find the equilibrium concentrations of each substance, use an ICE table. At equilibrium, the concentrations are: [A] = 0.450 mol/L, [B] = 1.45 mol/L, [C] = 0.450 mol/L, and [D] = 0.450 mol/L. The equilibrium constant (Keq) is calculated by dividing the product of the equilibrium concentrations of the products by the product of the equilibrium concentrations of the reactants.

Step-by-step explanation:

To find the equilibrium concentrations of each substance, we can use an ICE table. Initially, we have 1.00 mol of A and 1.00 mol of B. Since the mole ratio of A:B is 1:1, as [A] decreases by the amount x, the [B] increases by the same amount x. Therefore, at equilibrium, we will have [A] = 0.450 mol/L, [B] = 1.00 + 0.450 mol/L, [C] = 0.450 mol/L, and [D] = 0.450 mol/L.

To calculate the equilibrium constant (Keq), we use the concentrations at equilibrium. Keq is calculated by dividing the product of the equilibrium concentrations of the products ([C] * [D]) by the product of the equilibrium concentrations of the reactants ([A] * [B]). In this case, Keq = ([C] * [D]) / ([A] * [B]).

Using the equilibrium concentrations we found earlier, Keq = (0.450 * 0.450) / (0.450 * (1.00 + 0.450)). Simplifying this expression gives the value of Keq.