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Vapor pressure -- How does water still boil at 100°C in an open pot?
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[QUOTE="pisluca99, post: 6828365, member: 730550"] Ok, so at any constant temperature, vapor in the 'mass' of water is in equilibrium with the liquid water itself and appears in the form of bubbles, which however are able to rise (I suppose because the vapor is less dense than the liquid water). The vapor in these bubbles has a pressure which is the vapor pressure, at that particular temperature and once equilibrium has been established. At 100°C, the vapor pressure of the bubbles reaches atmospheric pressure and these become able to expand precisely because they overcome the atmospheric pressure pressing on them. These 'big' bubbles rise, generating the phenomenon of boiling. So essentially boiling is a 'rising of bubbles' which is much more visible and grosser than when the temperature is lower than 100 °C. I hope I finally found the solution. [/QUOTE]
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Vapor pressure -- How does water still boil at 100°C in an open pot?
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