External pressure on a liquid can paradoxically increase its vapor pressure, despite the common understanding that higher pressure makes it harder for the liquid to vaporize. This occurs because adding hydrostatic pressure raises the Gibbs free energy of the liquid, which increases the tendency for solvent molecules to escape into the vapor phase. The discussion highlights the importance of the Poynting correction and the relationship between pressure and Gibbs free energy, particularly at constant temperature. While higher external pressure typically requires higher temperatures for boiling, it can also lead to an increase in vapor pressure at constant temperature due to changes in molecular activity. Understanding these dynamics is crucial for grasping liquid-gas transitions and the effects of pressure on vaporization.