This is for "ammonia". The problem says that ammonia is a gas at room temperature. And that this tells us: "the fact that ammonia is a gas at room temperature tell us that vapor pressure of ammonia must be greater than atmospheric pressure". I know that for water, when the boiling point is reached, vapor pressure = atmospheric pressure and a phase change occurs (is the direction determined by the input or "taking away" of energy?). I thought that the pressure in a system could not be higher than 760mmHG though? So how is ammonia have a partial pressure higher than this and how does this tell us that we are dealing with a gas?