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Faraday's Law

According to Faraday's law, the amount of substance that undergoes oxidation-reduction reaction at the electrodes is directly proportional to the amount of electric current that the reaction is subjected to. Faraday constant is equal to the charge of one mol of electrons, and is numerically equal to 96500 coulombs. You probably remember `coulombs' from your physics undergraduate courses. The unit coulomb is related to the unit ampere (SI unit of current).

amperes x seconds = coulombs

current x time = charge

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