The molar concentrations for the reactants and products at equilibrium are found to be [HCl] = 0.80 M, [O2] = 0.20 M, [Cl2] = 3.0 M, and H2O = 3.0 M. What is the value of the equilibrium constant for this reaction? the complete reaction is 4HCl+O2=2Cl2+2H2O i got this answer but it tells me its wrong where did I go wrong with my computation pls check:
Kc= [3.0][3.0]2/[0.80]4[0.20]=329.58 pls kindly my computation
Both 3.0 values should be squared since both have coefficients of 2.
To calculate the equilibrium constant (Kc) for a reaction, you need to take into account the stoichiometry of the reaction. In this case, the balanced equation is:
4HCl + O2 → 2Cl2 + 2H2O
To determine the equilibrium constant, you need to raise the concentrations of the products (raised to the power of their stoichiometric coefficients) and divide by the concentrations of the reactants (raised to the power of their stoichiometric coefficients).
The correct calculation for the equilibrium constant in this case would be:
Kc = ([Cl2]^2 * [H2O]^2) / ([HCl]^4 * [O2])
Substituting the given values:
Kc = (3.0^2 * 3.0^2) / (0.80^4 * 0.20)
Kc = (9.0 * 9.0) / (0.4096 * 0.04)
Kc = 81 / 0.016384
Kc ≈ 4948.24
Therefore, the value of the equilibrium constant (Kc) for this reaction is approximately 4948.24.
From your computation, it seems like an error may have occurred in the denominator. Please recheck the values you used in the calculation and ensure that you raise them to the appropriate exponents based on the stoichiometry of the reaction.