What is the correct equilibrium constant expression for the following reaction? 3A2 = 2B3 when the reaction started with the initial concentrations of A2 = 3 M and B3 = 2 M and continued until the equilibrium concentrations of A2 = 2.5 M and B3 = 2.5 M

Question

Chemistry

Baby

23 August, 16:30

What is the correct equilibrium constant expression for the following reaction? 3A2 = 2B3 when the reaction started with the initial concentrations of A2 = 3 M and B3 = 2 M and continued until the equilibrium concentrations of A2 = 2.5 M and B3 = 2.5 M

+1

Answers (1)

Know the Answer?

Bradyn Cooley · Answer 1

Kc = [B₃]²/[A₂]³ = 0.40

Explanation:

3A₂ ⇄ 2B₃

Given at equilibrium = > [A₂] = 2.5 and [B₃] = 2.5

Kc = [B₃]²/[A₂]³ = (2.5) ² / (2.5) ³ = (2.5) ⁻¹ = 0.40