I understand why the vapor is cooled in such a scenario, because of the heat required to change states, but I don't fully understand why the state change even occurs if below the BP. Why does it seem that in many cases, atomization almost forces evaporation, minimizing the role of temperature?
I understand that air can naturally hold a certain amount of water, but I've never learned how this "humidity" concept applies to other solvents. Is there some kind of formula I can use to estimate how much of a particular solvent a particular volume of air can hold at room temperature, without the solvent being at boiling point? Or really any sort of math model to understand how atomization assists in evaporation below boiling point?