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9 Cards in this Set
- Front
- Back
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Charles Law
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CONSTANT PRESSURE
as Temp Increase, Volume Increases (DIRECT) V/T=K V1/T1=V2/T2 |
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Boyle's Law
(robert Boyle) |
CONATANT TEMPERATURE
(INVERSE) PTV PV=K P1V1=P2V2 |
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Gay Lussac's Law
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CONSTANT VOLUME
Temp Increases, Pressure Increases (DIRECT) P/T=K P1/T1=P2/T2 |
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Combined Gas Laws
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PV=K
V/T=K PV/T or P1V1/T1=P2V2/T2 P/T=K *PTV* |
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Dalton's Law of Partial
(DUH!) |
Total PRESSURE exerted by a mixture of gases = Sum of the partial Pressure of each gas
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Ideal Gas Laws
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PV=nRT .0821 LxATM/MOLxL
R= constant (.0821) P= pressure (atm) V= volume (l) one of everything n= # of moles no change! t= temperature (k) |
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Avogadro's Hypothesis
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EQUAL VOLUMES of any gas at the same TEMPERATURE and PRESSURE contain EQUAL # OF MOLES
DIFFERENT MASS... @stp= 6.02x10 to the 23 |
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Kinetic Molecular Theory of Gases
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Ideal gases:*molecules in random straight-line motion *have moleculesthat collide w/no net energy loss *molecules that have no attraction for one another *have molecules with no Volume....
Real Gases act like ideal gases when: high temps, low press, small molecules, PLIGHT, BBUUTT differ or deviate when LT and HP |
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Graham's Law of Diffusion
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MASS Increases, RATE Decreases
If more mass (bigger molecules) move slower than smaller molecules. r1/r2= m2/m1 m= mass r= rate |
