Underlying physics of partial pressures

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Gases in a mixture exist at partial pressures due to their individual contributions to the total pressure, which can vary based on temperature and volume. Moisture in the air can exist as superheated steam at temperatures below the boiling point due to low pressure conditions, suggesting it hasn't reached equilibrium. The distinction between evaporation and boiling is emphasized, with vapor being different from steam. An everyday example of slightly superheated steam is the pressurized steam above boiling water in a closed tea kettle. Understanding these concepts is crucial for grasping the underlying physics of gas behavior in mixtures.
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How do gases exist at partial pressures in a mixture. Moisture in the air is superheated steam, yet at a temperature well below atmospheric boiling point, implying that the moisture in the air is at very low pressures. How does it maintain this state?
 
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Maybe it hasn't reached equilibrium yet, that's got to be in the thermo book.
 
Evaporation is not (yet) boiling, vapours is not steam. An example of slightly superheated steam in everyday life is the pressurised steam over the boiling water in a closed tea kettle.
 
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