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one
- molecules (or atoms) of gases are continuously in motion
- always have NRG
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two
the volume of gas molecules is negligible compared to the volume of the container
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three
- the attractive and repulsive forces of gas molecules are negligible
- no affect on NRG transfer during a collision
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four
- as long as the temp remains constant, the average kinetic energy of the molecules is constant
- individual molecules can transfer NRG from one to another, but the average remains constant
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five
- the average kinetic energy is directly proportional to absolute temperature
- not dependent on the identity of gas
- all gases have the same average NRG at same temperature
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exceptions to rules
- 1. LOW TEMPS
- overall average kinetic E of the gas is low, so attractive/repulsive forces are not negligible (#3 in KMT doesn't hold true)
- 1. HIGH PRESSURE(greater than 10)
- low volume in system, so volume of molecules is no longer negligible (#2 in KMT)
- volume of molecule is significant
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to correct exceptions use Van der Waal's equation
- b = constant compensates for volume occupied by gas molecs
- a = contant that compensates for attractive/repulsive forces between molecs
a & b change based on the different gases
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