The solvation thermodynamics of cyclohexane in pure liquid phase and in wat
er is analyzed by means of the theoretical approach developed by Lee. The s
um of the work of cavity creation and the dispersive solute-solvent interac
tion energy reproduces well the experimental Gibbs energy values over the w
hole temperature range 5-100degreesC. This implies that the purely structur
al solvent reorganization is an exactly compensating process in both liquid
s. The dispersivesolute-solvent interaction energy is larger in magnitude i
n cyclohexane than in water, whereas the work of cavity creation is larger
in water than in cyclohexane. Therefore, both terms contrast the transfer o
f cyclohexane from pure liquid phase to water, determining its hydrophobici
ty. This mechanism qualitatively corresponds to that operative in the case
of benzene.