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)

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

first one is the correct answer

false

because it does not have the potential to be entirely used up