Gas Laws

P: pressure T: temperature V: volume n: moles MM: molar mass

STP: standard temperature and pressure

standard temperature: 0 ºC (= 273 K)

standard pressure: 1.000 atm

(1 atm = 760 mmHg = 760 torr = 101325 Pascals = 101.3 kPa = 29.92 in Hg = 14.7 lb/in²)

Temperature in Kelvin (TinK)

Kelvin/Celsius:

Volumes: 1000 cm³ = 1 dm³ = 1 liter = 1000 ml

Boyle's law: or therefore (temperature and amount are held constant)

Charles' law: therefore (when TinK and pressure and amount are held constant)

Gay-Lussac's law: therefore (when TinK and volume and amount are held constant)

Avogadro's Law: therefore (temperature and pressure are held constant)

Combined gas laws: therefore (when TinK and amount is held constant)

Dalton's law: when a gas is collected over water

Density: therefore (when TinK and )

Grahams Law:

Ideal gas law: (TinK, and R is 0.08206 )

Molar volume: at STP, 1 mole of a gas occupies 22.4 L and has Avogadro's number of particles (and the mass of one mole of the compound)