Final answer:
The equilibrium constant (Keq) for the reaction aA + bB <=> cC + dD is formed by dividing the product of the concentrations of products C and D (raised to their respective coefficients) by the product of the concentrations of reactants A and B (raised to their respective coefficients).
Step-by-step explanation:
Forming the Equilibrium Constant (Keq)
To form the equilibrium constant (Keq) for the reaction aA + bB <=> cC + dD, you would use the concentrations of the reactants and products. The Keq is given by the ratio of the products' concentrations to the reactants' concentrations, with each concentration raised to the power of its stoichiometric coefficient. The general formula for Keq is:
Keq = [C]^c [D]^d / [A]^a [B]^b
where [C], [D], [A], and [B] represent the molar concentrations of C, D, A, and B respectively. The exponents c, d, a, and b are the stoichiometric coefficients of the balanced chemical equation.
It's important to note that if the reaction were reversed, the equilibrium constant expression would also be reversed, and its value would be the reciprocal of the original reaction's Keq.