Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [I2]eq = 0.39 M, [HI]eq = 1.6 M. H2 (g) + I2 (g) ⇌ 2 HI (g)

Question

Grant Leblanc

Chemistry

10 January, 19:40

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [I2]eq = 0.39 M, [HI]eq = 1.6 M. H2 (g) + I2 (g) ⇌ 2 HI (g)

+4

Answers (1)

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Lennon Oliver · Answer 1

47

Explanation:

Let's consider the following reaction at equilibrium.

H₂ (g) + I₂ (g) ⇌ 2 HI (g)

The concentration equilibrium constant (Kc) is the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.

Kc = [HI]² / [H₂] * [I₂]

Kc = (1.6) ² / 0.14 * 0.39

Kc = 47