If K > 1, which statement about the equilibrium is correct?

If K > 1, which statement about the equilibrium is correct?

• A. The reverse reaction is favored
• B. Reactants are favored
• C. Products are favored
• D. The reaction stops at equilibrium

Answer: (C)

When K is greater than 1, the equilibrium lies toward the products, meaning the ratio of product concentrations to reactant concentrations at equilibrium is greater than one. This indicates more products than reactants are present when the system reaches balance, so the forward direction is favored at equilibrium. The larger the K value, the more complete the conversion to products. If K were less than 1, reactants would be favored instead. The idea that the reaction stops at equilibrium isn’t accurate, because at equilibrium forward and reverse rates are equal, so there’s no net change even though reactions still occur.

When K is greater than 1, the equilibrium lies toward the products, meaning the ratio of product concentrations to reactant concentrations at equilibrium is greater than one. This indicates more products than reactants are present when the system reaches balance, so the forward direction is favored at equilibrium. The larger the K value, the more complete the conversion to products. If K were less than 1, reactants would be favored instead. The idea that the reaction stops at equilibrium isn’t accurate, because at equilibrium forward and reverse rates are equal, so there’s no net change even though reactions still occur.