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Purdue University - Faraday's Law of Electrolysis
The amount of a substance consumed or produced at one of the electrodes in an electrolytic cell is directly proportional to the amount of electricity that passes through the cell.



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Special points of emphasis

Stoichiometry

Electrochemistry

DC Current

The extent of chemical change that occurs in an electrolytic cell is stoichiometrically related to the number of moles of electrons that pass through the cell. From the perspective of the voltage source and circuit outside the electrodes, the flow of electrons is generally described in terms of electrical current using the SI units of coulombs and amperes. It takes 96,500 coulombs to constitute a mole of electrons, a unit known as the faraday (F). This conversion is the linchpin of stoichiometric problem solving in electrochemistry: I tend to think the modern MCAT would provide this information. The test-writers do not seem to be inclined to care if you remember exactly how many coulombs of charge equals a mole of electrons, but in case I am wrong:

1 mol of electrons = 1 F = 96,500 C








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