Final answer:
A reaction is spontaneous under standard conditions when the equilibrium constant, K, is greater than 1, leading to a negative ΔG°.
Step-by-step explanation:
When considering whether a reaction is spontaneous under standard conditions, we look at ΔG°, the standard change in free energy. If ΔG° is negative, this indicates that the reaction is spontaneous in the forward direction. For spontaneity, we examine the equilibrium constant, K. Specifically, when K > 1, ΔG° is negative, demonstrating that the products are favored over the reactants when the system reaches equilibrium. Therefore, the reaction is spontaneous in the forward direction under standard conditions when K > 1. The correct answer to the question is a) >.