I have a question regarding the calculation of pressure. Not quite homework but just curious on how things work. If I had an enclosed 18 mL (1 mol H2O) container that is indestructible/incompressible filled with water, and boil it so that all the water turns into water vapour, I get 22.4 L of gas, or would the pressure force the gas to remain in liquid form in some way or another, or would I get some combination of the two? I'd also assume there'd be a large amount of pressure acting on the container as well due to expansion and whatnot. I'm not so sure the Ideal gas law applies in such a situation, as the gas is produced from a liquid and the other values don't quite apply... (as temperature increases, the pressure increases linearly?) Am I looking for a case of thermal expansion rather than gaseous expansion, or do both apply? I'm also unsure what else is relevant for this situation. Thanks in advance!