Vapor pressure is essentially only affected by the particular liquid and its temperature. However this is only an approximation.
So from possibilities provided I would choose.
temperature and intermolecular forces!
Vapor pressure describes the pressure of the vapor phase in equilibrium with the liquid phase of a substance. Intermolecular forces and temperature are the only factors that affect vapor pressure. For a given liquid, temperature is the only factor. Increasing temperature increases the average kinetic energy of the molecules, which increases the force of the collisions and the probability that a molecule will be able to overcome the intermolecular forces and escape into the vapor phase. The strength of the intermolecular forces also affects that probability: the weaker the forces, the easier it is for a molecule to break away. Surface area is not a factor because pressure is force per unit area. In other words, the area cancels out. Volume is not a factor because vaporization only occurs at the surface. Humidity can affect the pressure above water at a given instant, but it does not change the pressure that would result if equilibrium were established. Remember that vapor pressure can only be measured at equilibrium when there is no net evaporation or condensation.
mass of liquid
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For liquids, which of the following factors affect vapor pressure?
Check all that apply:
I answered and put that volume, temp. & intermolecular forces but got the question wrong. I think that surface area may be one. Please help explain. Thanks.