Final answer:
When transferring nonpolar molecules from water to a nonpolar solvent, TΔS is generally positive due to the increase in disorder (entropy). Consequently, ΔG tends to be negative, indicating that the process is energetically favorable and spontaneous.
Step-by-step explanation:
Considering the energetics of transferring nonpolar molecules from water to a nonpolar solvent, the factor TΔS (Temperature change in Entropy) is generally positive. This is because the nonpolar molecules are initially in an ordered state when dissolved in water due to water's highly polar nature, which enforces a certain structure on the nonpolar molecules. When these nonpolar molecules are transferred to a nonpolar solvent, they become more disordered, leading to an increase in entropy (ΔS). Since the entropy increases and temperature (T) is always a positive quantity in Kelvin, the product TΔS is positive.
With a positive TΔS, according to the Gibbs free energy equation, ΔG = ΔH - TΔS, the ΔG (change in Gibbs free energy) would be negative, assuming that the enthalpy change (ΔH) does not oppose this effect more strongly. A negative ΔG denotes a spontaneous process; hence, the transfer of nonpolar molecules from water to a nonpolar solvent is energetically favorable/