Why Does Water in a Boiling Container Not Boil?

AI Thread Summary
Water in an open-topped container suspended in boiling water can reach 100 degrees Celsius without boiling due to the balance of heat transfer and pressure. The boiling point of water is influenced by both temperature and atmospheric pressure; in this case, the pressure above the water in the open container allows it to remain in a liquid state despite reaching its boiling point. If the container is large enough or if heat is removed, the water may not receive sufficient energy to overcome the latent heat required for boiling. The discussion raises questions about the conditions affecting boiling, such as container size and initial temperatures. Ultimately, the phenomenon illustrates the complexities of heat transfer and phase changes in liquids.
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Homework Statement


If you suspend an open-topped container of water in a pot of boiling water, water in the inner container will reach 100 degrees C but will not boil. Why is this?


Homework Equations





The Attempt at a Solution

 
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Darned if I know! The question, as stated, makes no sense to me. The water in the open-topped container will eventually just mix with the other water, reach 100 degrees C and boil! Are there time constraints on this? Are you assuming that the heat causing the water in the pot is removed? In that case I suppose there are some conditions on the comparative size of the two containers and original temperature of the water in the container to allow the latent heat in the pot to cause an average temperature of 100 degrees for all the water but not sufficient additional heat to make up the 'heat of boiling' for all the water. But I don't think that's what's meant here.
 
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