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Vapor pressure -- How does water still boil at 100°C in an open pot?
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[QUOTE="Drakkith, post: 6828234, member: 272035"] Per wiki, vapor pressure: [I]is defined as the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system.[/I] So vapor pressure isn't something you measure, it is something you define. What you actually measure is the partial pressure of a gas, which in water's case is water vapor. So when you boil a pot of water, the vapor pressure of that water gradually rises because it is getting heated, but you wouldn't measure the vapor pressure since it is a defined quantity, not a measured one. A similar thing happens with the boiling point of a substance. If we changed the pressure around the pot of water instead of changing its temperature we would see that the boiling point changes as pressure falls or rises. And similar to vapor pressure, the boiling point isn't what you measure. You'd measure the temperature or pressure and then define the boiling point to be a certain temperature at a certain pressure, just like how vapor pressure is defined to be a certain pressure at a certain temperature. Note that by 'measure' I mean physically place a device to record some quantity, such as placing a pressure gauge or thermometer near the surface of the pot of water. [/QUOTE]
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Vapor pressure -- How does water still boil at 100°C in an open pot?
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