The reaction 2A(g) + B(g) ⇌ 3C(g) + D(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expressi

Question

The reaction 2A(g) + B(g) ⇌ 3C(g) + D(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

Accepted Answer

(0.75)^3 / [(0.50)^2 (0.25)]. At equilibrium, the concentration of D is 0.25 M, so the change in concentration of A and B can be calculated using stoichiometry. A decreases by 0.50 M (2:1 ratio with D), and B decreases by 0.25 M. The equilibrium concentrations are A = 0.50 M, B = 0.75 M, and C = 0.75 M. Substituting these values into the equilibrium constant expression gives option D.

The reaction 2A(g) + B(g) ⇌ 3C(g) + D(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

Solution

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