the principle that equal volumes of all gases at the same temperature and pressure contain the same number of molecules. Thus, the molar volume of all ideal gases at 0° C and a pressure of 1 atm. is 22.4 liters.

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Statement that, under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules (see Avogadro's number).

First proposed by the Italian scientist Amedeo Avogadro (1776–1856) in 1811, it became accepted с 1860. From the law, it follows that the volume occupied by one mole of gas (at standard conditions of 32 °F [0 °C] and 1 atmosphere of pressure) is the same for all gases (0.791 cubic feet [22.4 litres]).

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a statement that under the same conditions of temperature and pressure, equal volumes of different gases (gas) contain an equal number of molecules (molecule). This empirical relation can be derived from the kinetic theory of gases under the assumption of a perfect (ideal) gas (perfect gas). The law is approximately valid for real gases at sufficiently low pressures and high temperatures.

The specific number of molecules in one gram- mole of a substance, defined as the molecular weight in grams, is 6.02214179 × 1023, a quantity called Avogadro's number, or the Avogadro constant (Avogadro's number). For example, the molecular weight of oxygen is 32.00, so that one gram-mole of oxygen has a mass of 32.00 grams and contains 6.02214179 × 1023 molecules.

The volume occupied by one gram-mole of gas is about 22.4 l (0.791 cubic feet) at standard temperature and pressure (0° C, 1 atmosphere) and is the same for all gases, according to Avogadro's law.

The law was first proposed in 1811 by Amedeo Avogadro (Avogadro, Amedeo), a professor of higher physics at the University of Turin for many years, but it was not generally accepted until after 1858, when an Italian chemist, Stanislao Cannizzaro (Cannizzaro, Stanislao), constructed a logical system of chemistry based on it.

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Universalium. 2010.

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