Final answer:
If ΔG°' is positive and K'eq is less than 1.0, it means the reaction favors the reactants over the products at equilibrium and is non-spontaneous in the forward direction. Option 4.
Step-by-step explanation:
When the ΔG°' (standard free energy change) of a chemical reaction is positive and the equilibrium constant (K'eq) is less than 1.0 under standard conditions, it indicates that the reaction is not spontaneous in the forward direction. Instead, the reaction would be spontaneous in the reverse direction, meaning that the reactants would predominate over the products at equilibrium. This is because a positive ΔG°' value suggests that the reaction requires an input of energy to proceed
If ΔG°' is positive, it does not necessarily mean that work can be done under these conditions, nor does it suggest that the reaction is exothermic. Similarly, it does not mean that reactants and products are at equilibrium but rather that at equilibrium, the reactants are favored. Therefore, the correct answer to this question is that reactants predominate over products. Option 4.