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Hey guys, so Berkeley Review book says that atmospheric pressure affects boiling point but not vapor pressure.
From what I understand, vapor pressure (using water as the example) is the pressure exerted when the rate of evaporation equals the rate of condensation, and that pressure is created by the water molecules in the air above the liquid.
This must mean that at this equilibrium state, there's a certain amount/concentration of water gas molecules in the air just above the liquid surface. So I have 2 questions:
1) What determines the concentration of the water gas molecules in the air just above the liquid surface?
2) If atmospheric pressure increases, more force is pushing down on the air above the liquid surface - wouldn't this make it more difficult for the liquid molecules to evaporate, decreasing the amount of water gas molecules in that air space?
This is really screwing with my head, I don't even know what question to ask. Pls help
From what I understand, vapor pressure (using water as the example) is the pressure exerted when the rate of evaporation equals the rate of condensation, and that pressure is created by the water molecules in the air above the liquid.
This must mean that at this equilibrium state, there's a certain amount/concentration of water gas molecules in the air just above the liquid surface. So I have 2 questions:
1) What determines the concentration of the water gas molecules in the air just above the liquid surface?
2) If atmospheric pressure increases, more force is pushing down on the air above the liquid surface - wouldn't this make it more difficult for the liquid molecules to evaporate, decreasing the amount of water gas molecules in that air space?
This is really screwing with my head, I don't even know what question to ask. Pls help