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Water at standard atmospheric pressure cannot exist in the liquid state at temperatures greater than 212 F (100 C). If you continue to apply heat to a pot of boiling water, that energy is being used to make the phase transition from liquid to steam. Assuming you were able to contain the steam and water in the same container without increasing pressure (as pressure increases, so does the boiling/saturation temperature), the temperature of both the water and steam would remain 212 F until all the liquid water had evaporated. This mixture of liquid state and gas state water is called a saturated mixture, and can only exist at the boiling/saturation temperature for a given pressure.

Once this saturated mixture has completely become a vapor, the temperature of the steam will begin to increase as you continue to apply heat to it.

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Q: What happens if you continue to heat water after it becomes steam?
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