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### 9 Cards in this Set

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 Charles Law CONSTANT PRESSURE as Temp Increase, Volume Increases (DIRECT) V/T=K V1/T1=V2/T2 Boyle's Law (robert Boyle) CONATANT TEMPERATURE (INVERSE) PTV PV=K P1V1=P2V2 Gay Lussac's Law CONSTANT VOLUME Temp Increases, Pressure Increases (DIRECT) P/T=K P1/T1=P2/T2 Combined Gas Laws PV=K V/T=K PV/T or P1V1/T1=P2V2/T2 P/T=K *PTV* Dalton's Law of Partial (DUH!) Total PRESSURE exerted by a mixture of gases = Sum of the partial Pressure of each gas Ideal Gas Laws 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) Avogadro's Hypothesis EQUAL VOLUMES of any gas at the same TEMPERATURE and PRESSURE contain EQUAL # OF MOLES DIFFERENT MASS... @stp= 6.02x10 to the 23 Kinetic Molecular Theory of Gases 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 Graham's Law of Diffusion MASS Increases, RATE Decreases If more mass (bigger molecules) move slower than smaller molecules. r1/r2= m2/m1 m= mass r= rate