faraday

n.
The quantity of electricity that is capable of depositing or liberating 1 gram equivalent weight of a substance in electrolysis, approximately 9.6494 × 10⁴ coulombs.

[After Michael FARADAY.]

Symbol F. The electric charge carried by one mole of electrons or singly ionized ions, i.e. the product of the Avogadro constant and the charge on an electron (disregarding sign). It has the value 9.648 5309(29) × 10⁴ coulombs per mole. This number of coulombs is sometimes treated as a unit of electric charge called the faraday.

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fundamental constant. Symbol F. The product of the Avogadro constant and elementary charge, = 96 485.3383(83) C·mol^-1 with relative standard uncertainty 8.6 × 10^-8.
[Mohr P. J., Taylor B. N. CODATA Recommended Values of the Fundamental Physical Constants: 2002 (to be published)]
[Mohr P. J., Taylor B. N. Rev. Mod. Phys. Vol. 72:351-495 (2000)]
[Mohr P. Phys. Today Vol. 53:7, 11-16 (2000)]
[For latest recommended values, see http://physics.nist.gov/cuu/Constants/index.html]

To convert from faradays/sec to:

ampere (absolute), multiply by 96500.
ampere-hours, multiply by 26.8.
coulombs, multiply by 96490.

Convert:  Into:  ampere (absolute) ampere-hours coulombs

Result:

Related measurements:
faradays/sec

Michael Faraday	faraday flashlight