The total charge that passes through an electrolytic cell is given by the product of current and time.
An electrolytic cell is an electrochemical cell that utilizes an external source of electrical energy (voltage applied between two electrodes) to drive a chemical reaction that would not otherwise occur. This is in contrast to a galvanic cell, which itself is a source of electrical energy and the foundation of a battery.
The net reaction taking place in a galvanic cell is a spontaneous reaction, i.e. the Gibbs free energy remains negative, while the net reaction taking place in an electrolytic cell is the reverse of this spontaneous reaction, i.e. the Gibbs free energy is positive.
An electrolytic cell has three components: an electrolyte and two electrodes (a cathode and an anode). The electrolyte is usually a solution of water or other solvents in which ions are dissolved.
Molten salts such as sodium chloride can also function as electrolytes. When driven by an external voltage applied to the electrodes, the ions in the electrolyte are attracted to an electrode with the opposite charge, where charge-transferring (also called faradaic or redox) reactions can take place.
Only with an external electrical potential (i.e., voltage) of correct polarity and sufficient magnitude can an electrolytic cell decompose a normally stable, or inert chemical compound in the solution. The electrical energy provided can produce a chemical reaction which would not otherwise occur spontaneously.
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