In terms of spontaneity of reactions, when K is greater than 1, what can be inferred about the reaction?

When the equilibrium constant (K) is greater than 1, it indicates that at equilibrium, the concentration of the products is greater than the concentration of the reactants. This suggests that the forward reaction is favored, which aligns with the concept of spontaneity in a chemical reaction. A reaction is considered spontaneous when it proceeds in the direction of forming products without needing continuous external energy input.

In thermodynamic terms, a positive value for the Gibbs free energy change (ΔG) means that a reaction is non-spontaneous under the given conditions, while a negative ΔG indicates that a reaction is spontaneous. For a reaction at equilibrium, K > 1 corresponds to a negative ΔG, signifying that the reaction can occur spontaneously in the forward direction.

Therefore, if K is greater than 1, it can be inferred that the reaction is always spontaneous under standard conditions, as the formation of products is thermodynamically favored.