Faraday's laws of electrolysis

Faraday's laws state that the amount of chemical change at an electrode is proportional to electric charge, and that equal charges produce amounts proportional to substances’ chemical equivalent weights.

Faraday constant: The electric charge per mole of elementary charges, approximately 96,485 coulombs per mole. It converts the charge in the first law into moles of electrons.
Electric charge: A fundamental property of matter that determines its electromagnetic interactions. The first law uses total charge as the measure of electrolysis extent.
Michael Faraday: An English scientist whose work established foundational principles of electromagnetism and electrochemistry. His experiments on electrical decomposition yielded the two laws.
Electroplating: The deposition of a metal coating on an object by electrolysis. The laws predict coating mass from current and plating time.
Electrochemical series: A ranking of redox couples by their standard electrode potentials. It helps predict which electrode reactions compete with the reaction quantified by Faraday's laws.
Equivalent weight: The mass of a substance that supplies or reacts with one mole of charge equivalents. It determines how much different substances form under the same charge.
Electrode: An electrical conductor through which current enters or leaves an electrochemical system. The laws measure chemical change at these current-carrying surfaces.
William Whewell: An English polymath who introduced much of the terminology used in electrochemistry. He coined terms including electrode, ion, anode, and cathode for Faraday's work.
Electrorefining: The purification of a metal by dissolving and redepositing it electrolytically. The laws relate refining current to the amount of metal transferred.
Electrochemical cell: A system in which chemical reactions and electrical energy are coupled through electrodes and an electrolyte. The laws quantify matter transfer in the driven reactions of electrochemical cells.

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