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Boyle's Law

P₁V₁ = P₂V₂

Charles' Law

V₁ = V₂

T₁ T₂

T₁ T₂

Gay-Lussac's Law

P₁ = P₂

T₁ T₂

T₁ T₂

Combined Gas Law

P₁V₁ = P₂V₂

T₁ T₂

T₁ T₂

Ideal Gas Law

PV = nRT

Dalton's Law of Partial Pressure

Ptotal = P₁+P₂+P₃...

Graham's law of diffusion and effusion

Rate A = √molar mass B

Rate B √molar mass A

Rate B √molar mass A

Boyle's law deff

At constant temperature the pressure of a gas is inversely proportional to its volume.

Charles' law deff

At a constant pressure, the volume of a gas is directly proportional to its kelvin temperature.

Guy-Lussac's Law deff

at constant volume the pressure of a gas is directly proportional to its kelvin temperature.

Combined Gas Law deff

combines the laws of Boyle, Charles and Gay-Lussac; only the amount of gas is held constant.

Ideal gas law deff

an "ideal" gas would follow all of the assumptions of the Kinetic theory of gases perfectly (ideally). Real gases do not obey all of these assumptions perfectly, but many gases act very close to ideal.

Dalton's Law of Partial Pressure deff

at constant temperature and volume the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in the mixture.

Graham's law of diffusion and effusion deff

the tendency of molecules to move toward areas of lower concentration until the concentration is equal throughout is called diffusion.