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Gases
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A. Kinetic Molecular Theory
Particles in an ideal gas… have no volume. have elastic collisions. are in constant, random, straight-line motion. don’t attract or repel each other. have an avg. KE directly related to Kelvin temperature.
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B. Real Gases Particles in a REAL gas… Gas behavior is most ideal…
have their own volume attract each other Gas behavior is most ideal… at low pressures at high temperatures in nonpolar atoms/molecules
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C. Characteristics of Gases
Gases expand to fill any container. random motion, no attraction Gases are fluids (like liquids). no attraction Gases have very low densities. no volume = lots of empty space
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C. Characteristics of Gases
Gases can be compressed. no volume = lots of empty space Gases undergo diffusion & effusion. random motion
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K = ºC + 273 D. Temperature ºF ºC K -459 32 212 -273 100 273 373
Always use absolute temperature (Kelvin) when working with gases. ºF ºC K -459 32 212 -273 100 273 373 K = ºC + 273
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Kinetic Energy and Temperature
Kelvin Temperature scale is directly proportional to the average kinetic energy
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E. Pressure Which shoes create the most pressure?
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E. Pressure Barometer measures atmospheric pressure Mercury Barometer
Aneroid Barometer
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E. Pressure Manometer measures contained gas pressure U-tube Manometer
Bourdon-tube gauge
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E. Pressure KEY UNITS AT SEA LEVEL 101.325 kPa (kilopascal) 1 atm
760 mm Hg 760 torr 14.7 psi
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Standard Temperature & Pressure
F. STP STP Standard Temperature & Pressure 0°C K 1 atm kPa -OR-
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How pressure units are related:
1 atm = 760 mm Hg = kPa How can we make these into conversion factors? 1 atm kPa 760 mm Hg atm
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Guided Problem: 1. Convert 385 mm Hg to kPa 385 mm Hg x
2. Convert 33.7 kPa to atm 33.7 kPa 101.3 kPa x = kPa 760 mm Hg x 1 atm = .33 atm 101.3 kPa
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