Consider the reaction. Upper H subscript 2 upper o (g) plus upper C l subscript 2 upper O (g) double-headed arrow 2 upper H upper C l upper O (g). At equilibrium, the concentrations of the different species are as follows. [H2O] = 0.077 M [Cl2O] = 0.077 M [HClO] = 0.023 M What is the equilibrium constant for the reaction at this temperature?

0.089

Explanation:

Step 1:

The balanced equation for the reaction is given below:

H2O + Cl2O 2HClO

Step 2:

Data obtained from the question. This includes:

Concentration of H2O, [H2O] = 0.077 M

Concentration of Cl2O, [Cl2O] = 0.077 M

Concentration of HClO, [HClO] = 0.023 M

Equilibrium constant, K = ?

Step 3:

Determination of the equilibrium constant. This is illustrated below:

The equilibrium constant for the above reaction is given below:

K = [HClO]^2 / [H2O] [Cl2O]

K = (0.023) ^2 / (0.077 x 0.077)

K = 0.089

Therefore, the equilibrium constant for the above reaction is 0.089

Equilibrium constant for the reaction is 0.0892

Explanation:

This is the reaction of equilibrium

H₂O + Cl₂O ⇄ 2HClO

Eq 0.077M 0.077M 0.023M

Let's make the expression for Kc

Kc = [HClO]² / [Cl₂O]. [H₂O]

Kc = 0.023² / 0.077. 0.077 = 0.0892