Gaseous State

Boyle's law: the volume of a fixed mass of gas is inversely proportional to its pressure, provided the temperature remains constant.

Charles's law: the volume of a fixed mass of gas is directly proportional to its absolute temperature, provided the pressure remains constant. When temperature increase, pressure increases.

Avogadro's law: under the same conditions of temperature and pressure, the volume of gas is proportional to the amount of gas present.

IDEAL GAS EQUATION: pV=nRT

R is always taken to be 8.31 JK-1mol-1
pressure: Pa
Volume: m3
temperature: K

Basic assumptions of the kinetic theory as applied to an ideal gas:
1)the volume of the gas particles is negligible compared to the volume occupied by the whole gas.
2)the intermolecular forces of attraction between the molecules of the gas are negligible.
3)gas particles are in constant random motion. they continually collide with each other and pressure arises from the bombardment of these particles.
4) collisions between particles of the gas are perfectly elastic.

Evidence of deviation from ideality:
-many gases are termed real gases and they obey the equation only approximately at low pressure and high temperature.

GASES DEVIATE FROM IDEALITY AT HIGH PRESSURES AND LOW TEMPERATURES.

GASES BEHAVE MORE IDEALLY WHEN THEIR MOLECULES ARE SMALL AND NON-POLAR AND AT LOW PRESSURES AND HIGH TEMPERATURES.