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22 Cards in this Set
- Front
- Back
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Units of gas pressures |
1 Atm = 760 mmHg = 760 torr = 101.325 kPa |
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Standard temp and pressure |
273 K (0 deg Celsius) 1 Atm |
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Ideal gas |
Hypothetical gas with molecules that have no IMFs and occupy no volume |
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Ideal gas law |
PV = nRT |
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Density |
-Ratio of mass per unit volume of a substance - units: g/L
Density = PM/RT M= molar mass |
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Combined gas law |
P1V1/T1 = P2V2/T2 |
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How to find molar mass |
Find V2 Find the density (mass/V2) Multiply density by the volume |
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Avogadros principle |
All gases at a constant temp and pressure occupy volumes that are directly proportional to the number of moles of gas present
** as the # of moves of gas increases, the volume increases in direct proportion**
n/V= k n1/V1= n2/V2 |
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Boyle's Law |
- for a gas sample held at constant temp, the volume of the gas is inversely proportional to its pressure
PV = k P1V1=P2V2 |
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Charle's law |
- at constant pressure, the volume and absolute temp are directly proportional
V/T=k V1/T1= V2/T2 |
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Gay lussacs law |
At a constant volume, temperature and pressure are directly proportional to each other
P/T=k P1/T1=P2/V2 |
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Partial pressure |
Pressure exerted by each individual gas
P(partial)= (moles of gas/moles total)*P(total) |
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Daltons partial pressure law |
Total pressure = sum of partial pressures |
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Henry's law |
At various pressures, the concentration of a gas in a liquid increased or decreased
A= kh*Pa
A1/P1=A2/P2 =kh |
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Vapor pressure |
Pressure exerted by evaporated particles above the surface of a liquid |
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Kinetic molecular theory |
Explains the behavior of gases |
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Average KE of a gas particle |
- proportional to temp
KE= 1/2 mv^2 = 3/2 * kb*T
Kb= boltzmann constant (1.38*10^-23) |
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Root mean square speed |
Calc. avg KE and then calc the speed to which is corresponds
V= (3RT/M)^1/2 M= molar mass (kg/mol)
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Doffusion |
Movement of molecules from high to low concentration - particles with greater mass travel at a slower speed |
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Grahams law |
- isothermal and isobaric conditions
r1/r2= (M2/M1)^1/2
r= diffusion rates |
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Effusion |
Flow of gas particles under pressure from one compartment to another through a small opening |
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Van der waals equation of state |
Attempts to correct deviations from ideal gas law
(P + n^2a/V^2)(V-nb) =nRT |
