• Boyle's Law
• Amonton's Law
• Charles' Law
• Gay-Lussac's Law (law of combining volumes)
• Avogadro's Hypothesis
• Dalton's Law of Partial Pressures

Boyle's Law

	The Pressure (P) of a gas is inversely proportional to Volume (V) at constant Temperature (T) and moles of gas (n).
Robert Boyle	The product of pressure and volume of one measurement is equal to the product of the pressure and volume of another measurement.

Amonton's Law

• The Pressure of a gas is directly proportional to the Temperature (Kelvin) at constant V and n.

• Absolute Zero - The temperature (-273.15 C or 0 K) at which the volume and pressure of an ideal gas extrapolated to zero.
  • Definition proposed by Joseph Lambert in 1779

  

  where T_K is measured in Kelvin and T_C is measured in Celsius

Charles' Law

	The Volume of a gas is directly proportional to the Temperature (Kelvin) at constant P and n.
Jacques-Alexandre- César Charles

Gay-Lussac's Law  (law of combining volumes)

	The ratio of the volumes of gases consumed or produced in a chemical reaction is equal to the ratio of simple whole numbers (coefficients in the balanced equation). e.g.  Carbon monoxide combines with oxygen in a 2:1 ratio by volume
Joseph Louis Gay-Lussac

Avogadro's Hypothesis

	The Volume of a gas is directly proportional to the moles of the gas, n at constant P and T. The hypothesis that equal volumes of different gases at the same temperature and pressure contain the same number of particles.
Amadeo Avogadro

Dalton's Law of Partial Pressures

The total pressure of a mixture of gases is equal to the sum of the partial pressures of the various components. Partial Pressure - The fraction of the total pressure of a mixture of gases that results from one component of the mixture. This Law can be used to correct the amount of water vapor picked up when a gas is collected by displacing water. Vapor Pressure - The pressure of the gas that collects above a liquid in a closed container.

John Dalton

Next:  "Ideal Gas Equation"