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The Avogadro constant, commonly denoted N A [1] or L, [2] is an SI defining constant with an exact value of 6.022 140 76 × 10 23 mol −1 (reciprocal moles). [3] [4] It is this defined number of constituent particles (usually molecules, atoms, ions, or ion pairs—in general, entities) per mole and used as a normalization factor in relating the amount of substance, n(X), in a sample of a ...
Avogadro constant: 6.022 140 76 ... and is strongly dependent on how those units are defined. For example, the atomic mass constant is exactly known ...
For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant. The law is named after Amedeo Avogadro who, in 1812, [ 2 ] [ 3 ] hypothesized that two given samples of an ideal gas, of the same volume and at the same temperature and pressure, contain the same ...
For any substance, the number density can be expressed in terms of its amount concentration c (in mol/m 3) as = where N A is the Avogadro constant. This is still true if the spatial dimension unit, metre, in both n and c is consistently replaced by any other spatial dimension unit, e.g. if n is in cm −3 and c is in mol/cm 3 , or if n is in L ...
Using simple algebra on equations , , and yields the result: = or =, where stands for the Boltzmann constant. Another equivalent result, using the fact that =, where n is the number of moles in the gas and R is the universal gas constant, is: =, which is known as the ideal gas law.
Using the modern values for the Avogadro constant 6.022 14 × 10 23 mol −1 and for the volume of a gram-molecule under these conditions of 22.4146 × 10 6 mm 3, the modern value is 2.687 × 10 16, instead of Stoney's 10 18.
The mass of a silicon atom could be determined using the Avogadro project and using the Avogadro constant, it could be linked directly to the kilogram. [65] Concerns that the authors of the proposal had failed to address the impact of breaking the link between the mole, kilogram, dalton, and the Avogadro constant (N A) have also been expressed.
where is the molar mass constant, is the Avogadro constant, [5] and () is the experimentally determined molar mass of carbon-12. [ 6 ] The relative isotopic mass (see section below) can be obtained by dividing the atomic mass m a of an isotope by the atomic mass constant m u yielding a dimensionless value .