Answer :
Therefore, the equilibrium constant (K) for the given reaction is approximately 0.047.
To calculate the equilibrium constant (K) for the given reaction:
3A + 2B ⇌ 3C
The equilibrium constant expression is defined as the ratio of the product concentrations raised to their stoichiometric coefficients divided by the ratio of the reactant concentrations raised to their stoichiometric coefficients.
K = [C]^3 / ([A]^3 * [B]^2)
Plugging in the given concentrations at equilibrium:
A] = 2 M
[B] = 3 M
[C] = 1.5 M
K = (1.5)^3 / ((2)^3 * (3)^2)
K = 3.375 / (8 * 9)
K = 3.375 / 72
K ≈ 0.047 (rounded to 2 significant figures)
The equilibrium constant, approximately 0.047, represents the ratio of the product concentrations to the reactant concentrations at equilibrium. In this case, the equilibrium constant suggests that the forward reaction is favored, as the product concentration is greater than the reactant concentration. However, the actual interpretation of the magnitude of K and the direction of the reaction depends on the context and the specific reaction conditions.
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