23 terms

# gas laws

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pressure
Force/Area
newton
1kg * 1m/s^2
pascal
1N/1m^2
standard temperature and pressure
STP = 1atm and 0 degrees celcius
kinetic-molecular theory
gas particles are in constant rapid, random motion. Also particles of a gas are very far apart relative to their size
Boyle's law
P1V1=P2V2
Charle's law
V1/T1=V2/T2
Gay-Lussac's law
P1/T1=P2/T2
V=kn k=22.41
ideal gas
a theoretical gas that follows all of these laws perfectly
ideal gas law
PV=nRT
diffusion
gases travel in all directions and mix quickly with molecules of gases in the air in a process.
effusion
the passage of gas particles through a small opening
Graham's law of diffusion
va/vb=Root(Mb/Ma)
Gay-Lussac's law of combining volumes
if pressure and temperature are kept constant, gases react in volume proportions that are whole numbers
Partial pressure
the pressure of each gas in a mixture
Dalton's law of partial pressure
P(total)=P(a)+P(b)+P(c)
Ideal gas constant
R=8.314LkPa/molK
Atmosphere of pressure
1atm=760mm Hg
Bar
1bar= 101,325 Pa
Millimeter of Mercury
1mm Hg= 133.322 Pa
Pounds per Square inch
1 psi = 6.892 x 1000
Torr
1 torr = 133.322