Kinetic theory of gases

Mole

A measure of the amount of a substance

Avogadro constant

N^a = 6.02 × 10²³

N^a = nN

n : amount of gas in moles

N : number of molecules

Molar mass

Mass per mole of the gas:

M = molecular mass / 1000

Pressure

P = Force / area

Boyle’s law

For a fixed mass at constant temperature, pressure is inversely proportional to the volume

Absolute zero

The temperature at which the energy of the particles is at its lowest

Kinetic theory of an ideal gas

A theoretical gas composed of randomly moving particles with negligible volume, no intermolecular forces and where collisions are perfectly elastic

Ideal gas equations

PV = nRT

PV = NkT

PV = 1/3 x Nm(rms)²

Kinetic theory of gas pressure

The force due to random hits are equal and opposite to the mean rate of change of the molecule’s momentum:

PV = 1/3 x Nm(rms)²

P = 1/3 x density(rms)²

Root mean square speed

A square root of the averaged squared speed of all the particles:

C² = /(C1)²(C2)²(C3)² x 1/2

Mean kinetic energy of molecules

Mean KE = ½ x m(rms)²