sorry but that doesn't change my understanding of why this occurs.
Why do liquids with a high vapour pressure dry out faster?
like in the attached file there is some molecules turning to gas and some turning to liquid. if the rate of this happening is the same the it is said to reach the liquids vapour pressure.
But i don't get how pressure outside this system has an effect on this equilibrium (e.g. replace the container from a place of high pressure and put it in a room where it is subject to atmospheric pressure)
like if a jug of a volatile liquid is placed on the table and is subject to atmospheric pressure. then if atmospheric pressure is 1 atm and the vapour pressure of the liquid is say, 2 (I don't know the units as i really dont understand this) would it not be the case that atmospheric pressure is pushing down on the molecules causing them to come closer together. If the vapour pressure is lower, say 0.5 then those molecules could diffuse more relative to the atmospheric pressure pushing down on them and more would turn to a gas than condense to a liquid.