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Unformatted text preview: • At high pressures, and low volumes, the intermolecular distances can become quite short, and attractive forces between molecules becomes significant o Neighboring molecules exert an attractive force, which will minimize the interaction of molecules with the container walls. And the apparent pressure will be less than ideal (PV/RT will thus be less than ideal). • As pressures increase, and volume decreases, the volume of the gas molecules becomes significant in relationship to the container volume o In an extreme example, the volume can decrease below the molecular volume, thus PV/RT will be higher than ideal (V is higher) • At high temperatures, the kinetic energy of the molecules can overcome the attractive influence and the gasses behave more ideal o At higher pressures, and lower volumes, the volume of the molecules influences PV/RT and its value, again, is higher than ideal •...
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- Fall '10
- Chemistry, ideal behavior