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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: 6827571, member: 730550"] Thanks a lot for your replies, but I still have my doubt. Originally, the vapor pressure experiment was performed in a closed container: in this case it is observed how, over time and at a constant temperature, the partial pressure of the vapor on the liquid increases progressively, until it reaches a constant value, which would be the saturated vapor pressure. Once this condition is reached, the number of water particles that condense is equal to the number of water particles that vaporize and there is no more mass change in the liquid. If we now open the container, always at the same temperature, it happens that the water molecules in the vapor phase tend to escape into the surrounding environment, and the previously established liquid-vapor equilibrium no longer exists, so much so that the mass of The water evaporates until it disappears completely: this should mean that, always at that specific temperature, the saturated vapor pressure is not reached, as in the case of a closed container. Therefore, at a certain temperature, if the vessel is open, a lower vapor pressure will be reached than with saturated steam. Consequently, this also happens at 100 °C and the water should not boil, unless the container is closed in such a way that the saturated vapor pressure, as well as atmospheric pressure, can be reached. What am I doing wrong? Sorry for the boredom. [/QUOTE]
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Vapor pressure -- How does water still boil at 100°C in an open pot?
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