The diagram above shows the interactions between the solute and solvent molecules of a sample in both the dissolved and undissolved states. Based on the diagram, which of the following statements is true concerning the sign of the overall change in Gibbs free energy (ΔG), the net change in enthalpy (ΔH), and the change in entropy (ΔS) for the solute dissolution?

ΔS is positive, but the signs of ΔG and ΔH cannot be determined without additional information.
ΔG is negative, because the net ΔH is negative and the ΔS is positive.
ΔG is positive, because the net ΔH is negative and the ΔS is positive.
ΔG is negative, because the net ΔH is positive and the ΔS is positive.