A principle stated in 1811 by the Italian chemist Amadeo Avogadro (1776–1856) that equal volumes of gases at the same temperature and pressure contain the same number of molecules regardless of their chemical nature and physical properties. This number (Avogadro's number) is 6.023 × 1023. It is the number of molecules of any gas present in a volume of 22.41 L and is the same for the lightest gas (hydrogen) as for a heavy gas such as carbon dioxide or bromine. Avogadro's number is one of the fundamental constants of chemistry. It permits calculation of the amount of pure substance in a mole, the basis of stoichiometric relationships. It also makes possible determination of how much heavier a simple molecule of one gas is than that of another; as a result the relative molecular weights of gases can be ascertained by comparing the weights of equal volumes. Avogadro's number (conventionally represented by “N” in chemical calculations) is now defined to be the number of atoms present in 12 grams of the carbon-12 isotope (one mole of carbon-12) and can be applied to any type of chemical entity.See Mole.
