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In physics and chemistry, the Faraday constant (named after Michael Faraday) is the magnitude of electric charge per mole of electrons.[1] It has the currently accepted value:[2][3]
The constant F has a simple relation to two other physical constants:
where
NA is the Avogadro constant, and e is the elementary charge or the magnitude of the charge of an electron. This relation is true because the amount of charge of a mole of electrons is equal to the amount of charge in one electron multiplied by the number of electrons in a mole.
The value of F was first determined 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.[4] Research is continuing into more accurate ways of determining the interrelated constants F, NA, and e.
Contents
Other Common Units of Faraday's Constant
- 96.485 kJ per volt gram equivalent
- 23.061 kcal per volt gram equivalent
Faraday unit of charge
Related to Faraday's constant is the "Faraday", a unit of electrical charge. It is much less common than the coulomb, but sometimes used in electrochemistry.[5] One Faraday of charge is the magnitude of the charge of one mole of electrons, i.e. 96,485.3399(24) C.
Expressed in Faradays, the Faraday constant F equals "1 faraday of charge per mole".
This Faraday unit is not to be confused with the farad, an unrelated unit of capacitance.
See also
References
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