Question

At a certain temperature, the equilibrium constant for the chemical reaction shown is 2.72��10-3. At equilibrium, the concentration of ab is 3.025 m, the concentration of bc is 2.325 m, and the concentration of ac is 0.260 m. Calculate the concentration of b at equilibrium. The chemical reaction is: ab(aq) + bc(aq) ������ ac(aq) + 2b(aq)

Answer 1

The concentration of b at equilibrium is approximately 0.043 M.

Step-by-step explanation:

Given the equilibrium constant (Keq) for the reaction ab(aq) + bc(aq) → ac(aq) + 2b(aq) is 2.72 × 10^-3 and the concentrations of ab, bc, and ac at equilibrium are 3.025 M, 2.325 M, and 0.260 M respectively, we can calculate the concentration of b at equilibrium.

1. First, we need to write the expression for the equilibrium constant (Keq). In this case, it is Keq = [ac][b]^2 / [ab][bc].
2. Using the given concentrations, we can substitute the values into the expression to solve for [b].
3. Plugging the values into the expression Keq = [0.260][b]^2 / [3.025][2.325], we can solve for [b] and find that the concentration of b at equilibrium is approximately 0.043 M.