In physics and chemistry, the Faraday constant (named after Michael Faraday) is the magnitude of electric charge per mole of electrons.[1] While most uses of the Faraday constant, denoted F, have been replaced by the standard SI unit, the coulomb, the Faraday is still widely used in calculations in electrochemistry. 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.
Other Common Units of Faraday's Constant
- 96.484 kJ per volt gram equivalent
- 23.061 kcal per volt gram equivalent
See also
- Farad, unit of capacitance
- Michael Faraday
- Faraday cage
- Faraday Efficiency
- Faraday's law of electrolysis
- Faraday's law of Electromagnetic induction
References
- ^ The term "magnitude" is used in the sense of "absolute value": The charge of an electron is negative, but F is always defined to be positive.
- ^ CODATA 2006
- ^ Mohr, Peter J.; Taylor, Barry N. (2005). "CODATA recommended values of the fundamental physical constants: 2002". Rev. Mod. Phys. 77 (1): 1–107. doi:.
- ^ NIST Introduction to physical constants
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