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Definition
| Particles in all forms of matter are in constant motion |
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| There is a lot of empty space between the particles so gases are compressible and expandable; there are no attractive or repulsive forces between the gas particles; take shape and volume of container; move in constant motion until they collide; they are all elastic |
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Definition
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| Volume and pressure relationship |
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Definition
| More volume= less pressure |
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Definition
| More temperature, more pressure |
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Definition
| More moles= more pressure |
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| Boyle's Law (Pressure and Volume) |
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Definition
| P1V1=P2V2 (temp is constant) |
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| Charle's Law (temperature and volume) |
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Definition
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| Lussac's Law (Pressure and temperature) |
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| Avogadro's Law (moles and volume) |
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Definition
Molar Mass= dRT/P
d= density |
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| Dalton's Law of Partial Pressure |
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Definition
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Term
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Definition
X1 = P1/Ptotal
X1= mole fraction
P1= first pressure
Ptotal= total pressure |
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Term
| Kelvin Temperature of a gas |
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Definition
KEavg = 3/2RT
Universal gas constant= 8.31 J/Mol x K
(NOTE: To find J/MOLECULE, divide by 6.02 x 10^23) |
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Term
| Root Mean Square Velocity |
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Definition
Velocity= Square root of 3RT/M
R= Constant (8.31)
M= kg/mol of a single gas particle
T= temperature (K) |
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Term
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Definition
| The rate at which a gas escapes through a tiny hole |
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| Rate of the Effusion of a Gas |
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Definition
(Rate 1/Rate 2) = Square root of M2/M1
Rate1= atom with low mass
Rate2= atom with more mass
M= masses
(Example: rates of He to N= square root of 28 over square root of 4) |
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