At high temperatures,Cl₂ breaks down into chlorine atoms: Cl₂ (g) ⇌ 2 Cl (g)
If K_c =2.68 at a given temperature,find the equilibrium concentrations of Cl₂ and Cl if the initial concentration of Cl₂ is 1.05 M.

Question

Quizplus · Accepted Answer

The equilibrium constant expression for the reaction is:K_c = [Cl]^2/[Cl₂]Substituting the given values into the expression, we get:2.68 = [Cl]^2/[Cl₂][Cl]^2 = 2.68[Cl₂][Cl] = 1.64[Cl₂]^1/2The initial concentration of Cl₂ is 1.05 M, so the initial concentration of Cl is 0.At equilibrium, let the change in concentration of Cl₂ be -x and the change in concentration of Cl be +2x.Therefore, the equilibrium concentrations of Cl₂ and Cl are:[Cl₂] = 1.05 - x[Cl] = 2xSubstituting these expressions into the equilibrium constant expression, we get:2.68 = (2x)^2/(1.05 - x)Solving for x, we get:x = 0.288Therefore, the equilibrium concentrations of Cl₂ and Cl are:[Cl₂] = 1.05 - x = 0.482 M[Cl] = 2x = 1.14 M

At High Temperatures,Cl2 Breaks Down into Chlorine Atoms: Cl2 (G)⇌

At High Temperatures,Cl₂ Breaks Down into Chlorine Atoms: Cl₂ (G)⇌