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23 terms

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

Avogadro's law

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=8.314L**kPa/mol**K

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