Answer:
Therefore, the equilibrium constant (K) for the given reaction is 23.7.
Step-by-step explanation:
To calculate the equilibrium constant (K), we need to use the law of mass action. The law of mass action states that the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients is equal to the equilibrium constant.
The balanced chemical equation is:
4HCl(aq) + O2(g) + 2Cl2(g) + 2H₂O(g) ⇌ 4ClH0.5(aq)
The stoichiometric coefficients indicate that the reaction involves a one-to-one ratio of reactants to products. Therefore, we can write:
K = [ClH0.5]^4 / [HCl]^4 [O2] [Cl2]^2 [H2O]^2
Substituting the given concentrations into the expression, we get:
K = [(0.883/2)^4] / [(0.302)^4 (0.109) (0.883)^2 (0.166)^2]
Simplifying the expression and calculating, we get:
K = 23.7
Therefore, the equilibrium constant (K) for the given reaction is 23.7.