In an open system the vapor pressure of a liquid, if it is not boliling is less thatn the atmospheric pressure.
As the temperature of the liquid increases, the vapor pressure increases. When the vapor pressure equals the atmospheric pressure the molecules of liquid escape and the liquid boils. The temperature at which this happens is the boiling point.
Vapor pressure is directly related to the temperature of the liquid. user: in an open system, the vapor pressure is equal to the outside air pressure.
Explanation;
-As the temperature of a system increases, the average kinetic energy of the molecules increases in both the liquid and gas phases.
-A higher average kinetic energy facilitates the escape of molecules from the liquid phase into the gas phase. At the same time, the rate of return of gas phase molecules to the liquid also increases. A new equilibrium point is reached at a higher gaseous vapor pressure. The increase in vapor pressure with temperature is exponential.
