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Faraday constant
From Wikipedia, the free encyclopedia
In physics and chemistry, the Faraday constant is the amount of electric charge per mole of electrons. The Faraday constant was named after British scientist Michael Faraday, and is widely used in calculations in electrochemistry.
It has the symbol F, and is related to the charge on an individual electron by
- F = NAe,
where NA is Avogadro's number (approximately 6.02×1023 mole−1) and e is the elementary charge, the magnitude of the charge on an electron (approximately 1.602×10−19 coulombs per electron).
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[1]. Research is continuing into more accurate ways of determining F, and thereby NA. [Source: NPL Annual Review 1999]
- F = 96 485.3383(83) coulomb/mole
Peter J. Mohr, and Barry N. Taylor, CODATA Recommended Values of the Fundamental Physical Constants: 2002, Rev. Mod. Phys. vol. 77(1) 1-107 (2005)
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