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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: 6828353, member: 730550"] From what I understood, at any constant temperature, an equilibrium is established between vapor and liquid, therefore this means that bubbles form in the 'mass' of water, which however cannot rise because the atmospheric pressure does not allow it. However, at 100 degrees, the vapor that makes up the bubbles, always in equilibrium with the liquid, reaches such a pressure as to overcome the atmospheric pressure and the bubbles can rise. If the container is closed, this equilibrium is also established on the surface of the liquid, while if the container is open, this equilibrium cannot occur on the surface because the vaporized water molecules escape into the atmosphere. Having said that, namely that the vapor of the bubbles is in equilibrium with the liquid, I would say that the correct answer is b, i.e. there are vapor bubbles in equilibrium with the surrounding liquid. [/QUOTE]
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Vapor pressure -- How does water still boil at 100°C in an open pot?
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