A mixture of 0.577 M H_2O , 0.314 M Cl_2O , and 0.666 M HClO are enclosed in a vessel at 25°C .
H_2O(g) + Cl_2O(g) <> 2 HOCl (g) Kc = 0.0900 at 25°C
1. Calculate the equilibrium concentrations of each gas at 25°C .

Equilibrium Concentration of H₂O(g)  = 0.803

Equilibrium Concentration of Cl₂O(g)  = 0.540

Equilibrium Concentration of HOCl (g) = 0.214

Explanation:

Given;

                H₂O(g)  +   Cl₂O(g) <-------> 2HOCl (g)

I                 0.577        0.314                   0.666                

C               - x              -x                        +2x

E             0.577 - x     0.314 - x               0.666 +2x

Equilibrium Concentration of H₂O(g) = 0.577 - (- 0.226) = 0.803

Equilibrium Concentration of Cl₂O(g) = 0.314 - (- 0.226) = 0.540

Equilibrium Concentration of HOCl (g)  = 0.666 +2(- 0.226) = 0.214

Thus, from the result it can be seen that at equilibrium, the reactants are favored.

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