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Avogadro constant

The Avogadro constant (symbols: L, NA), also called the Avogadro number is the number of "entities" (usually, atoms or molecules) in one mole,[1][2] that is the number of carbon-12 atoms in 12 grams (0.012 kg) of unbound carbon-12 in its ground state. The current best estimate of this number is: [3]

N_A = (6.022 \, 141 \, 79\pm 0.000 \, 000 \, 30)\,\times\,10^{23} \mbox{ mol}^{-1} \,

The value of the number was first indicated by Johann Josef Loschmidt, who in 1865, computed the number of particles in one cubic centimetre of gas in standard conditions. The term Loschmidt constant is thus more correctly applied for this latter value, which can be said to be proportional to the Avogadro number. However, in German language literature, "Loschmidt constant" is used to refer to both this usage, as well as the number of entities in a mole.


History and etymology

The Avogadro constant is named after the early nineteenth century Italian scientist Amedeo Avogadro, who is credited (1811) with being the first to realize that the volume of a gas (strictly, of an ideal gas) is proportional to the number of atoms or molecules. The French chemist Jean Baptiste Perrin in 1909 proposed naming the constant in honor of Avogadro. American chemistry textbooks picked it up in the 1930s followed by high school textbooks starting in the 1950s.[4]

Loschmidt: Measuring the Avogadro Number

Avogadro never attempted to measure the constant: the numerical value was first estimated by the Austrian physicist Johann Josef Loschmidt in 1865 using the kinetic theory of gases.[5] In German-speaking countries, the constant is sometimes referred to as the Loschmidt constant or Loschmidt's number, but what Loschmidt actually measured is the number of particles per unit volume of an ideal gas, i.e. the number density of particles in an ideal gas. Thus, the term Loschmidt constant is more appropriate to the number of particles per unit of gas, Symbol: no:[6]

n_\circ = \frac{p}{k_B T} \,

equal to (2.686 7774 ± 0.000 0047) × 1025 m−3 at 273.15 K and 101.325 kPa with kB the Boltzmann constant, T the temperature and p the pressure.

This constant is related to the Avogadro constant by the relation:

R = N_Ak_B  \,

with kB the Boltzmann constant hence

N_A = \frac{n_\circ R T}{p}  \,

However, in German scientific literature, the term Loschmidt constant is used ambiguously - it often refers to what has come to be known as Avogadro number.[7] However, Boltzmann had first used the term for the sense in which Loschmidt had measured it - the number of particles in an unit volume of gas. Thus, its use in referring to the related Avogadro number leads to confusion and is usually deprecated. For the same reason, sometimes the Avogadro Number is denoted as L as opposed to NA in German texts.[5]

Standardization of the mole

Before 1960, there were conflicting definitions of the mole, and hence of the Avogadro number (as it was known at the time), based on 16 grams of oxygen: physicists generally used oxygen-16 while chemists generally used the "naturally occurring" isotope ratio. Switching to 12 grams of carbon-12 as the basis ended this dispute and had other advantages.[8]

At this time, the Avogadro number was defined as the number of atoms in 12 grams of carbon-12, that is as a dimensionless quantity, while a mole was defined as one Avogadro number of atoms, molecules or other entities. When the mole entered the International System of Units (SI) in 1971 as the base unit of amount of substance, the definitions were interchanged: what had previously been a number became a physical constant with the unit of reciprocal moles (mol−1).


The Avogadro constant can be applied to any substance. It corresponds to the number of atoms or molecules needed to make up a mass equal to the substance's atomic or molecular mass, in grams. For example, the atomic mass of iron is 55.847 g/mol, so NA iron atoms (i.e. one mole of iron atoms) have a mass of 55.847 g. Conversely, 55.847 g of iron contains NA iron atoms. The Avogadro constant also enters into the definition of the unified atomic mass unit, u:

1 \ u = \frac{1}{N_A} \ g = (1.660 \, 538\, 86 \pm 0.000\, 000\, 28) 10^{-24} \ g

Additional physical relations

Because of its role as a scaling factor, the Avogadro number provides the link between a number of useful physical constants when moving between the atomic scale and the macroscopic scale. For example, it provides the relationship between:

R = k_BN_A =   8.314 \, 472 \, \pm \, 0.000 \, 015 \, \mbox{J}\cdot\mbox{mol}^{-1}\mbox{K}^{-1}\,
in J mol−1 K−1
  • the Faraday constant F and the elementary charge e:
F = N_Ae =   96 \, 485.3383 \, \pm \,0.0083 \,\, \mbox{C}\cdot\mbox{mol}^{-1} \,
in C mol−1

Measurement of the Avogadro constant

  A number of methods can be used to measure the Avogadro constant. One modern method is to calculate the Avogadro constant from the density (ρ) of a crystal, the relative atomic mass (M), and the unit cell length (a) determined from x-ray crystallography.[9] Very accurate values of these quantities for silicon have been measured at the National Institute of Standards and Technology (NIST) and used to obtain the value of the Avogadro constant:

N_A  =  \frac{8M}{a^3\rho} \,.
based on silicon.[10]

See also

References and notes

  1. ^ International Union of Pure and Applied Chemistry Commission on Physiochemical Symbols Terminology and Units (1993). Quantities, Units and Symbols in Physical Chemistry (2nd Edition). Oxford: Blackwell Scientific Publications. ISBN 0-632-03583-8. Retrieved on 2006-12-28.  International Union of Pure and Applied Chemistry Commission on Quantities and Units in Clinical Chemistry; International Federation of Clinical Chemistry Committee on Quantities and Units (1996). "Glossary of Terms in Quantities and Units in Clinical Chemistry (IUPAC-IFCC Recommendations 1996)". Pure Appl. Chem. 68: 957–1000. Retrieved on 2006-12-28.
  2. ^ International Union of Pure and Applied Chemistry Commission on Atomic Weights and Isotopic Abundances (1992). "Atomic Weight: The Name, Its History, Definition and Units". Pure Appl. Chem. 64: 1535–43. Retrieved on 2006-12-28.
  3. ^ CODATA (2006).
  4. ^ How and When Did Avogadro's Name become Associated with Avogadro's Number? Jensen, William B. J. Chem. Educ. 2007 84 223. Link
  5. ^ a b Bader, Alfred; Parker, Leonard. "Joseph Loschmidt, Physicist and Chemist". Physics Today Online (March 2001). Retrieved on 2006-12-28.
  6. ^ National Institute of Standards and Technology (February 2006). Fundamental physical constants: Physico-chemical constants. Retrieved on 2006-12-28.
  7. ^ S. E. Virgo (933). "Loschmidt's Number". Science Progress 27: 634-649.
  8. ^ Bureau international des poids et mesures (March 2006). Unit of amount of substance (mole). Retrieved on 2006-12-28.
  9. ^ Mineralogy Database (2000-2005). Unit Cell Formula. Retrieved on 2007-12-09.
  10. ^ Mineralogy Database (2000-2005). Unit Cell Dimensions for Silicon. Retrieved on 2007-12-09.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Avogadro_constant". A list of authors is available in Wikipedia.
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