When the equilibrium constant (K) is greater than 1, it indicates that the products of a chemical reaction are favored over the reactants at equilibrium. This often means that at equilibrium, the concentration of the products is significantly greater than that of the reactants.
The reason for this lies in the nature of chemical reactions. A K value greater than 1 signifies that the reaction tends to proceed in the forward direction. As the reaction progresses, reactants convert to products until a point of balance, or equilibrium, is achieved.
At equilibrium, the rate of the forward reaction (formation of products) equals the rate of the reverse reaction (formation of reactants). However, because K is greater than 1, there are more product molecules than reactant molecules at this balance. In essence, this indicates a strong tendency for the reaction to favor product formation.
Overall, when K > 1, you can conclude that the equilibrium shifts toward the side of the products, meaning that at equilibrium, the reaction lies predominantly on that side.