IDEAL GAS LAW

- 1811, Amadeo Avogadro

- a statement that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules

- approximately valid for real gases at sufficiently low pressures and high temperatures.

V = kn

V1/n1 = V2/n2

V - volume

n - no. of gas in mol

specific number of molecules in one gram-mole of a substance, defined as the molecular weight in grams, is 6.02214076 × 10²³

from this law is that if samples of any gas are compared that have the same volume, temperature and pressure, then they will all have the same number of molecules in them.

Ideal gases are essentially point masses moving in constant, random, straight-line motion

PV = nRT

P - pressure

V - Volume

n - no. of mol

R - gas constant (8.31 J/K mol or 0.082 L atm/K mol)

T - temperature

molecules of a gas are in a state of perpetual motion in which the velocity of each molecule is completely random and independent of that of the other molecules.

A gas is composed of molecules that are separated by average distances that are much greater than the sizes of the molecules themselves. The volume occupied by the molecules of the gas is negligible compared to the volume of the gas itself.

The molecules of an ideal gas exert no attractive forces on each other, or on the walls of the container.

The molecules are in constant random motion, and as material bodies, they obey Newton's laws of motion.

Collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved. 

The average kinetic energy of the gas molecules is directly proportional to the absolute temperature.