Final answer:
When K = 1, ΔG° is 0, meaning that the reaction is at equilibrium under standard conditions and neither reactants nor products are favored.
Step-by-step explanation:
When K = 1, ΔG° is 0 and the reaction is at equilibrium under standard conditions. At this point, the system has reached a state where neither reactants nor products are favored, meaning that the forward and reverse reactions occur at the same rate, leading to a dynamic balance. The equilibrium constant K indicates the ratio of product concentrations to reactant concentrations at equilibrium, and ΔG° represents the standard free energy change associated with a chemical reaction.
If ΔG° < 0, the equilibrium constant K will be greater than 1, indicating a spontaneous reaction in the forward direction where products are favored. Conversely, if ΔG° > 0, K will be less than 1, and the reverse reaction is spontaneous, favoring reactants. Therefore, when K equals 1, ΔG° equals to 0, indicating that the system is at equilibrium and no net reaction is occurring.