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Introductory Physics Homework Help
Do you need to account for the water heating up to the boiling point?
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[QUOTE="haruspex, post: 6834765, member: 334404"] I fail to see how this produces a different answer from opinion 1. Each molecule that evaporates has to reach a certain energy to escape and carries that energy away with it. If you start with mass M and mass m evaporates the energy transferred is MC∆T+mL. If I pour a glass of water from the tap and leave it to stand (humidity being less than 100%) it will gradually evaporate. In the process it will get colder and absorb heat from the surrounding. Even if I perfectly insulate it, it will do that until its temperature drops to the dew point. Once there, evaporation matches condensation. I suspect that the state of boiling is widely misunderstood. It is not that all the molecules simultaneously reach the energy required to escape. Rather, the temperature reaches the point at which the SVP matches the atmospheric pressure, allowing bubbles of vapour to form within the water. This greatly increases the surface area, allowing the rate of vaporisation to match the rate of heat input. [/QUOTE]
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Introductory Physics Homework Help
Do you need to account for the water heating up to the boiling point?
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