I read in my Chemistry workbook that: "At higher temperatures, vapour pressure increases as more energy is provided to the liquid molecules, allowing them to escape into the gas phase." At the boiling point, all energy is gone into breaking bonds and to convert liquid phase molecules into gaseous. Why does it say at higher temperatures, more molecules escape into the gas phase? Once past the boiling point, wouldn't all the original liquid molecules of the original sample be converted to the gas state by then? Also, does Dalton's Law of Partial Pressure only apply if all the initial gas constituents occupy the same volume and are all placed in a container of the same volume?