How Does a Vacuum Influence Water Evaporation Rates at 322K?

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SUMMARY

The discussion focuses on the influence of a vacuum on water evaporation rates at a temperature of 322K. It establishes that the evaporation rate is contingent upon the difference between the vapor pressure of water and the actual pressure of water vapors above the liquid. In a vacuum, where the pressure of water vapors is effectively zero, the net evaporation is maximized. The conversation also highlights the importance of maintaining a consistent temperature and vacuum level to optimize evaporation rates.

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  • Understanding of vapor pressure and its relationship to temperature.
  • Knowledge of vacuum pressure measurements, specifically inHg.
  • Familiarity with the principles of phase changes in liquids.
  • Basic grasp of thermodynamic concepts related to evaporation.
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  • Research the equations governing vapor pressure, particularly the Clausius-Clapeyron equation.
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Telruc
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I am new to this site and would like to find some equations for water evaporation? I would like to understand more fully how placing water in a vacuum effects the rates at which it will evaporate?

Any help would be greatly appreciated
 
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The evaporation rate depends on several factors. The one that is related to your question is the difference between the "vapor pressure" of water and the actual pressure of the water vapors above the liquid.
There is a net evaporation as long as the pressure of the water vapors above the liquid is less than the vapor pressure.
In a vacuum this difference is maximum (pressure of the water vapors=0)

The "vapor pressure" is a characteristic of the liquid and depends on temperature.
 
So under a Vacuum you are assisting the evacuation of molecules on the surface of the water and allowing more molecules to vaporize. Assuming you could keep the water at a consistent temp of 322K, a consistent vacuum of 27.5 inHg., over a surface area of 24 Inches. What would the evaporation rate be?
 

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