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as each molecule of water evaporates it takes heat with it, lowering the temperature of the surrounding water, so it takes time before every molecule evaporates.

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Q: When heating a sample of pure water to the boiling point why doesn't all of the water instantly vaporize when you reach the boiling point?
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Why doesnt the all the water instantly vaporize when you reach the boiling point?

The boiling point is the temperature where a substance BEGINS to vaporize. So all of the water doesn't necessarily need to boil off instantly. To vaporize, molecules of water need to have energy. Only at the boiling point do they have enough energy to boil away, and when they do, they carry this energy with them. This means that a constant supply of heat for a certain period of time is needed for all water in a sample to boil off.


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