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In a closed system, liquids are at equilibrium with their vapor phase. Water vapor at equilibrium with its liquid phase exerts a pressure of 3.2 KPa at 25 oCentigrade. Applying a vacuum reduces vapor pressure. This disturbs equilibrium. To re-establish equilibrium, more water must evaporate. A constant vacuum will prevent attainment of equilibrium and produce continuous vaporization.. resulting in drying.

2007-05-25 20:35:32 · answer #1 · answered by CC 2 · 0 0

i'd honeslty say serach this online.

Google it

basically though...when you create a "vacuum" the pressure drops....and at said temperature......things that should be liquid turn into vapor and are sucked off.

I just threw out my notebook that has the energy balance but i remember there was a sign error that caused a project i was doing to not work out...... and i found it online pretty fast.

2007-05-26 04:23:40 · answer #2 · answered by My name is not bruce 7 · 0 0

A vacuum lowers the temperature at which a liquid will evaporate. For more information, consult a chemical engineering text.

2007-05-26 03:15:52 · answer #3 · answered by cattbarf 7 · 0 0

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