In a closed system, water vapor would have nowhere to go and atmospheric pressure would not be a factor. It would reach dynamic equilibrium with only water vapor.
But in an open system, I think that the water vapor would be forced back down into the liquid state by the atmospheric pressure until it is heated to the boiling point, at which the water vapor would equal or exceed the atmospheric pressure allowing water vapor particles to escape.
Is my understanding correct?
It just doesn’t seem to be how it works since water vapor can evaporate and escape even before it reaches the boiling point. Or instead, would only fast enough particles be able to overcome and escape the atmospheric pressure and the boiling point would only be when practically all of the water particles have reached that speed
I need help understanding in-depth the process of evaporation and vaporization on a particulate level. Starting from very basic chemistry might help.