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Faraday constant
| Faraday constant | |
|---|---|
.jpg) Michael Faraday, the constant's namesake | |
Common symbols | F |
| SI unit | coulomb per mole (C/mol) |
| In SI base units | s⋅A⋅mol−1 |
Derivations from other quantities | F = eNA |
| Value | 9.64853321233100184×104 C⋅mol−1 |
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: F = q/n; it is expressed in units of coulombs per mole (C/mol). As such, it represents the "molar elementary charge",[1] 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,[1] 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):
- F = e × NA
- = 1.602176634×10−19 C × 6.02214076×1023 mol−1
- = 9.64853321233100184×104 C⋅mol−1.
- ^ a b Newell, David B.; Tiesinga, Eite (2019). The International System of Units (SI). NIST Special Publication 330. Gaithersburg, Maryland: National Institute of Standards and Technology. doi:10.6028/nist.sp.330-2019. S2CID 242934226.
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