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A flask partially full of liquid water is heated to boiling and capped cold water is poured over the flask. The water boils even more vigorously explain

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  1. The boiling point of a solvent is the temperature at which the vapor pressure of the solvent equals atmospheric pressure (the pressure surrounding the solvent in the case of a capped flask). So, a boiling solution means the vapor pressure = 760 mm Hg if the atmospheric pressure is 760 mm. Now, we cap the flask, run cold water over the outside. What happens. The cold water reduces the temperature of the boiling water. (P1/T1) = (P2/T2) which means that the pressure inside the flask is reduced significantly, the vapor pressure is reduced also; however, the vapor pressure of the liquid STILL IS as high or higher than the pressure above it and that is the definition of boiling. The solution continues to boil. This is the same phenomenon that exists when boiling water on top of Pike's Peak. The atmospheric pressure is lower than at the base of the mountain and water boils at a lower temperature; i.e., when the vapor pressure of the water is less than 760 mm.

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