Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [Cl2]eq = 0.39 M, [HCl]eq = 1.6 M. H2 (g) + Cl2 (g) ⇌ 2 HCl (g) 8.7 * 10-22.1 * 10-229473.4 * 10-2

Kc = 47

Explanation:

From the given equation,

H₂ (g) + Cl₂ (g) ⇌ 2 HCl (g)

The equilibrium constant for the above reaction, can be written as the product of the concentration of product raised to the power of stoichiometric coefficients in a balanced equation of dissociation divided by the product of the concentration of reactant raised to the power of stoichiometric coefficients in the balanced equation of dissociation.

Hence,

Kc = [HCl (g) ]² / [ Cl₂ (g) ] [ H₂ (g) ]

From the question,

[HCl (g) ] = 1.6 M

[ Cl₂ (g) ] = 0.39 M

[ H₂ (g) ] = 0.14 M

Now, putting it in the above equation,

Kc = [HCl (g) ]² / [ Cl₂ (g) ] [ H₂ (g) ]

Kc = [ 1.6 M ]² / [ 0.39 M ][ 0.14 M ]

Kc = 47