Why Does Water in a Boiling Container Not Boil?

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SUMMARY

The discussion centers on the phenomenon where water in an open-topped container suspended in boiling water reaches 100 degrees Celsius without boiling. Participants express confusion regarding the conditions under which this occurs, particularly questioning the influence of heat transfer and the size of the containers. It is established that the water in the inner container does not boil due to the lack of sufficient heat to overcome the latent heat of vaporization, despite reaching the boiling point. The conversation highlights the importance of understanding heat dynamics in thermodynamic systems.

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  • Understanding of thermodynamics principles
  • Knowledge of latent heat and heat transfer mechanisms
  • Familiarity with boiling point concepts
  • Basic physics of heat conduction and convection
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  • Study heat transfer methods: conduction, convection, and radiation
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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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