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Faraday constant

Physical constant: Electric charge of one mole of electrons

Summary

Physical constant: Electric charge of one mole of electrons

Field	Value
name	Faraday constant
image	Michael_Faraday_(1791-1867).jpg
caption	Michael Faraday, the constant's namesake
unit	coulomb per mole (C/mol)
symbols	F
baseunits	s⋅A⋅mol−1
dimension	wikidata
derivations
value

In physical chemistry, the Faraday constant (symbol F, sometimes stylized as ℱ) is a physical constant defined as the quotient of the total electric charge (q) by the amount (n) of elementary charge carriers in any given sample of matter: it is expressed in units of coulombs per mole (C/mol). As such, it represents the "molar elementary charge", that is, the electric charge of one mole of elementary carriers (e.g., protons). It is named after the English scientist Michael Faraday. Since the 2019 revision of the SI, the Faraday constant has an exactly defined value, the product of the elementary charge (e, in coulombs) and the Avogadro constant (NA, in reciprocal moles): :

Derivation

The Faraday constant can be thought of as the proportionality factor between the charge in coulombs (used in physics and in practical electrical measurements) and the amount of substance in moles (used in chemistry), and is therefore of particular use in electrochemistry, particularly in electrolysis calculations. Because the elementary charge is exactly , and there are exactly entities per mole, the Faraday constant is given by the product of these two quantities: : : :

The value of F was first determined in the 1800s by weighing the amount of silver deposited in an electrochemical reaction, in which a measured current was passed for a measured time, and using Faraday's law of electrolysis. Until about 1970, the most reliable value of the Faraday constant was determined by a related method of electro-dissolving silver metal in perchloric acid.

Other common units

96.485 kJ per volt–gram-equivalent
23.061 kcal per volt–gram-equivalent
26.801 A·h/mol

Faraday – a unit of charge

Related to the Faraday constant is the "faraday", a unit of electrical charge. Its use is much less common than of the coulomb, but is sometimes used in electrochemistry. One faraday of charge is the charge of one mole of elementary charges (or of negative one mole of electrons), that is, : 1 faraday = F × 1 mol = = N0 × e = .

Where N0 is Avogadro's number, the unitless counterpart to NA. Conversely, the Faraday constant F equals 1 faraday per mole. (The farad is an unrelated unit of capacitance, ).

References

Newell, David B.. (2019). "The International System of Units (SI)". National Institute of Standards and Technology.
[http://physics.nist.gov/cuu/Constants/historical1.html NIST Introduction to physical constants]
IUPAC. (1976). "Status of the Faraday constant as an analytical standard". Pure and Applied Chemistry.
[https://books.google.com/books?id=r-Qpy0KQayIC&pg=PA51 ''Foundations of Physics, Volume 2'', by R. S. Gambhir, 1993, p. 51]

Wikipedia Source

This article was imported from Wikipedia and is available under the Creative Commons Attribution-ShareAlike 4.0 License. Content has been adapted to SurfDoc format. Original contributors can be found on the article history page.

electrochemical-concepts physical-constants michael-faraday units-of-electrical-charge molar-quantities quotients

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