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A measure of how much the volume of matter decreases under pressure

Boyle&#039;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&#039;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&#039;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 law

The relationship PV = nRT which describes the behavior of an ideal gas

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&#039;s hypothesis


Partial pressure


Dalton&#039;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 +...


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


The process that occurs when a gas escapes through a tiny hole in its container

Graham&#039;s law of effusion

The rate of effusion of a gas is inversely proportional to the square root of its molar mass; this relationship is also true for the diffusion of gas Rate A / Rate B = sqr root(molar mass B / molar mass A)

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