The boiling point is defined as the temperature where the vapour pressure is equal to external pressure. So it will always rise with pressure.realitysickness said:Hi DrDu, do you mind responding to my earlier question: "My only question remains then: given the information you just stated, for situations where temperature is not a constant, why are the boiling point temperatures of a liquid higher at higher pressures?
No, it does not. Ideal gases don't know of each other. So when in the gas phase, the energy of the vapour will only depend on temperature, but not on pressure. The energy of the liquid on the other hand is slightly increased due to compression. So the energy a molecule needs to go from the liquid to the gas phase decreases. For real gases there are slight deviations from ideality at high pressures, but these are weaker than the energy change due to pressure of the liquid.OldYat47 said:Increasing the pressure in a gaseous atmosphere above a liquid increases the amount of energy needed for individual molecules to escape to a vapor state. The first effect is much smaller than the second.