Question

Consider the reaction 2 A(g) ⇄ B(g) + C(g) K = 0.035 A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to reach equilibrium. What is the equilibrium concentration of A?

Answer 1

To find the equilibrium concentration of A after adding 0.50 moles of A to the equilibrium mixture, use the ICE method and the equilibrium constant expression to solve for x, the change in concentration.

Step-by-step explanation:

To calculate the equilibrium concentration of A after disturbing the equilibrium by adding 0.50 moles of A to the mixture, we should apply the ICE (Initial, Change, Equilibrium) method. Initially, we have 1.0 mole of B and C each in a 1.0 liter container, and an added 0.50 moles of A. When equilibrium is re-established, [A] is reduced by a certain amount x, while [B] and [C] are increased by x according to stoichiometry. Using the equilibrium constant K, we can set up an equation to solve for x and subsequently find the equilibrium concentration of A, B, and C.

Given the equilibrium constant K = 0.035 and stoichiometry of the reaction 2 A(g) ⇄ B(g) + C(g), we can write the equilibrium constant expression as K = [B][C] / [A]2. Plugging in the equilibrium concentrations and solving for [A] will provide the desired concentration of A at equilibrium. The ICE table helps in determining the initial concentrations, the changes in concentration, and the final equilibrium concentrations.