We examine the following reaction at 250C: PCl5(g) ⇌ PCl3(g) + Cl2(g). At equilibrium we find [PCl5] = 3.4 x 10-5 M, [PCl3] = 1.3 x 10-2 M, and [Cl2] = 1.0 x 10-4 M. Calculate the equilibrium constant, Kc.reaction.
(a) 26 (b) 5.1 (c) 2.8 x 10-4 (d) 0.038
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(c) 2.8*10^4
The answer is 0.038. Substituting into the equilibrium expression, you have K = (0.013*0.0001)/(0.000034)
To calculate the equilibrium constant, Kc, for the given reaction, we need to use the concentrations of the reactants and products at equilibrium. The equilibrium constant is defined as the ratio of the products to the reactants, with each concentration raised to the power of its coefficient in the balanced chemical equation.
The balanced chemical equation for the reaction is:
PCl5(g) → PCl3(g) + Cl2(g)
The concentrations at equilibrium are:
[PCl5] = 3.4 x 10^-5 M
[PCl3] = 1.3 x 10^-2 M
[Cl2] = 1.0 x 10^-4 M
Using the concentrations in the equation, the equilibrium constant expression (Kc) can be written as:
Kc = [PCl3] * [Cl2] / [PCl5]
Substituting the given concentrations into the equation, we get:
Kc = (1.3 x 10^-2 M) * (1.0 x 10^-4 M) / (3.4 x 10^-5 M)
Simplifying the expression:
Kc = 3.82 x 10^-2
Rounding to the appropriate number of significant figures, the equilibrium constant, Kc, is approximately 0.038.
Therefore, the answer is (d) 0.038.