Final answer:
When ΔG°' is positive and K'eq is less than 1.0, the reaction is spontaneous in the reverse direction, indicating that the formation of reactants from products is favored.
Step-by-step explanation:
When the ΔG°' of a chemical reaction is positive and the equilibrium constant (K'eq) is less than 1.0 under standard conditions, this means that the reaction is spontaneous in the reverse direction. This is because a positive ΔG°' indicates that under standard conditions, the free energy of the reactants is lower than that of the products, and the reaction does not proceed spontaneously towards forming more products.
Therefore, the reaction is not at equilibrium, and it is not spontaneous in the forward direction. For a reaction to be spontaneous in the forward direction, the ΔG°' would need to be negative, indicating that the products are favored and K'eq would be greater than 1.0.