### Boyle's Law

For a given mass of a gas at constant temperature, the volume of the gas varies inversely with pressure P1 xV1 = P2 x V2

### Charle's Law

The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant V1/T1 = V2/T2

### Gay-Lussac's Law

The pressure of a gas is directly proportional to the Kelvin temperature if the volume is constant P1/T1 = P2/T2

### Combined Gas Law

The law that describes the relationship among the pressure, temperature, and volume of an enclosed gas (P1 x V1) / T1 = (P2 x V2) / T2

### Ideal gas

A gas that conforms to the ideal gas law. Conforms exactly to all of the assumptions of the kinetic theory

### Ideal gas constant

The constant in the ideal gas law, has the symbol R and the value 8.31 (L x KPa)/(K x Mol)

### Real gas

Differ from ideal gases at low temperatures and high pressures, do not exactly meet the assumptions of the kinetic theory

### Avogadro's hypothesis

Equal volumes of gases at the same temperature and pressure contain equal numbers of particles

### Dalton's law of partial pressure

At constant volume and temperature the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases P total = P1 + P2 + P3 +...

### Diffusion

The tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout