I am a high school student and I am very confused in a topic about "vapor pressure of liquid". Why doesn't a change in atmospheric pressure affect vapor pressure? I think intuitively that vapor pressure should decrease on increasing the atmospheric pressure. Say I have an open bowl of water at temperature T and 1atm pressure and the vapor pressure at temperature T is P1. Now I increase the atmospheric pressure over the bowl keeping the temperature same (we can do it by pushing more air by some external means towards liquid surface). Because a higher atmospheric pressure is pushing on the liquid, doesn't that mean less evaporation and hence less vapor pressure for same temperature?
But on the other hand, I also think that vapor pressure is defined when there is an equilibrium between the liquid and vapor phase of water and equilibrium constants are only affected by temperature. Therefore, if vapor pressure changes with a change in external pressure, than it would mean the equilibrium constant would have to change?
Please prove me wrong (if I am) with some intuitive explanation at a high school level.