Scharles said:isn't mean that the ratio of [products] / [reactants] remain unchanged after the system is adjusted to equilibrium ??
The equilibrium constant (K) is a numerical value that represents the ratio of product concentrations to reactant concentrations at equilibrium for a given chemical reaction.
The equilibrium constant K is calculated by taking the concentrations of the products, raised to the power of their coefficients, and dividing it by the concentrations of the reactants, also raised to the power of their coefficients. This calculation is only valid when the reaction is at equilibrium.
A high value of equilibrium constant K indicates that the reaction favors the formation of products at equilibrium, meaning the products are more stable than the reactants. A low value of equilibrium constant K indicates that the reaction favors the formation of reactants at equilibrium, meaning the reactants are more stable than the products.
The equilibrium constant K is affected by changes in temperature. An increase in temperature will generally favor the endothermic reaction, causing an increase in the value of K, while a decrease in temperature will favor the exothermic reaction, causing a decrease in the value of K.
Yes, the equilibrium constant K is affected by changes in concentration or pressure of the reactants or products. However, the value of K itself does not change, but the value of the concentrations used in the calculation of K will change, resulting in a new value for K.