Faraday (unit)

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The faraday , also called faraday in English , named after the British physical chemist Michael Faraday , is a historical unit of the amount of charge . It is defined as the amount of charge that one gram equivalent of an ion removes from an electrolyte solution :

1 Faraday = N A · e · 1 mol = 96 485.339 9 Coulomb

It was mainly used in electrochemistry . In 1933, for example, the National Bureau of Standards Journal of Research stated : “the difference in free energy […] is 0.5 volt faraday per equivalent.” And “F (Faraday constant) = 23.067 g-cal. 15 (international volt equivalent) −1 ".

Individual evidence

  1. ↑ National Bureau of Standards: Journal of Research , Vol. 9 (1932/33), p. 368 or p. 681, ISSN  0091-1801 ( digitized by Google ).