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Vapor pressure -- How does water still boil at 100°C in an open pot?
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[QUOTE="256bits, post: 6827529, member: 328943"] Not exactly correct about the open container. It is a more or less general statement that seems to be completely true but is not quite actually, considering that from our everyday experience water does evaporate. Sometimes we should be wary of such general statements often repeated, and re-analyze if it considers all conditions. The air has a percentage of water vapour within it. At any given day, we listen to the weather report and most of the time they give a temperature and the relative humidity. The relative humidity is the ratio of actual amount of water vapour within the air to that which could be within the air at that temperature. On a day with 100% relative humidity ( which doesn't happen all that often ), the water vapour is at the saturation pressure, meaning that the liquid-vapour equilibrium is reached ( as you have put it ) for any container, or any body of water, open to the atmosphere, where the body of water is at the same temperature as the air. Dew will form on surfaces when the temperature of the air falls near or below the saturation temperature near the surface. So even if completely open to the 'rest' of the atmosphere, condensation onto a surface is an example of the vapour-liquid moving in the opposite direction - ie from the vapour state to the liquid state. [/QUOTE]
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Vapor pressure -- How does water still boil at 100°C in an open pot?
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