Here, we obtain ∆𝐸 = 12.6 kJ • mol which is the energy difference between melting transition and dispersion of NCs. We can attribute the ∆𝐸 to the strength of ligand-solvent interaction (i.e., alkanoate-chloroform interaction) if we assume the melting process completely releases ligand-ligand interaction. Nevertheless, ∆𝐸 is small as compared to 𝐸 of 330 ~ 350 • mol This corroborates the assumption that dispersion and melting of NCs are intrinsically analogous thermodynamic transitions that are governed by the ligand-ligand interaction . Meanwhile, ∆𝑆 is obtained as 0.97 kJ • mol • K which approximates ∆𝑆 . This indicates that the conformational entropy changes of the ligands during melting and dispersion transitions are also at the same order.