Answer:
Step-by-step explanation:
The equilibrium constant (Kc) is a measure of the relative concentrations of the reactants and products at equilibrium for a given chemical reaction. It is defined as the ratio of the product concentrations raised to their stoichiometric coefficients, to the reactant concentrations raised to their stoichiometric coefficients. For a general reversible reaction
aA + bB <=> cC + dD
The equilibrium constant is defined as:
Kc = [C]^c [D]^d / [A]^a [B]^b
where [X] represents the concentration of species X (in molarity units), and the superscripts on the concentrations represent the stoichiometric coefficients of the species in the balanced equation for the reaction.
The reaction quotient (Qc) is similar to the equilibrium constant, but it is calculated using the concentrations of the reactants and products at a given point in time, rather than at equilibrium. The reaction quotient is also defined as the ratio of the product concentrations raised to their stoichiometric coefficients, to the reactant concentrations raised to their stoichiometric coefficients, and is calculated using the same equation as Kc, but with the concentrations at a specific point in time, rather than at equilibrium.
Qc = [C]^c [D]^d / [A]^a [B]^b
It can be used to predict the direction of reaction depending on the sign of Qc, Kc.
If Qc < Kc, the reaction will shift in the direction of products.
If Qc > Kc, the reaction will shift in the direction of reactants
If Qc = Kc, the reaction is at equilibrium.
If you want to know more about equilibrium reaction you can check on Le Chatelier's principle.