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When pure liquid water is left in a closed container, some of it will evaporate, even if it's not boiling. The evaporated water (vapour) will build up until an equlibrium is reached between the rate of evaporation (liquid -> vapour) and the rate of condensation (vapour -> liquid). At that point, the pressure of the water vapour is called the 'vapour ...


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Water has an interesting property in which on being heated its temperature will not increase beyond its boiling point unless all the water has converted to vapour. This extra energy provided is used in converting water to vapour at the same temperature and is called latent heat of vaporization. So as long as you keep the temperature above the boiling point ...


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Water evaporates at all temperatures above freezing point, but weather condenses it back into rain, which finds its way back into the oceans. If atmospheric water was lost into space, at a greater rate than cosmic water entered the Earth's atmosphere, after sufficient undetermined time, all the ocean's waters may be lost.


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The boiling point of saturated saline solution is around 108.7°C, so you need a temperature at least as high as this. I wonder if you are mixing up the temperature required with the amount of energy required. As long as we keep the temperature above the boiling point we can evaporate an arbitrarily large amount of water, but of course it will require an ...


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Well, I am not at expert and also am new so my answer could be unsatisfying or wrong. But here I go: The temperature should be around 99.97 C for the water to boil. To boil all the water and evaporate the water in all the oceans, the same temperature of 99.97 C could work if the equal amount of heat is applied to all the molecules. That is, if each molecule ...


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Are you studying basic thermodynamics? Because your question is exactly what people learn in the first few classes of this subject. First Law of Thermodynamics tells us that every joule of energy from the burner will act to increase the system's internal energy.note 1 Also, the total volume of your system is constant (isochoric process). We need only to use ...


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The issue is not "equilibrium" - the issue is boiling. During boiling, there is explicitly NO equilibrium: the water wants to get out of the liquid phase, and into the vapor phase. The temperature of the liquid is sufficiently high that liquid can evaporate below the surface (strictly speaking the temperature must be slightly above boiling for that, as the ...


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The reason behind the hissing sound is that the temperature of the water droplet is much lower than the hot surface. As soon as the water droplet's base touches the hot surface it quickly evaporates but still the top part of the droplet is in liquid state and there is an opposition to th water-vapour coming from below. As the water-vapour couldn't vertically ...



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