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Electrolytic cell



Additional recommended knowledge

Contents

Electrolytic cells are composed of a vessel used to do electrolysis, containing electrolyte, usually a solution of water or other solvents capable of dissolving various ions into solution, and a cathode and anode. The electrolyte in the cell is inert unless driven by external voltage into a redox reaction with the anode and cathode. The term literally means a cell that splits up or loosens ions.

Galvanic cells compared to electrolytic cells

In contrast, a galvanic cell, also known as a voltaic cell, generates electricity using two metals that have different reaction potentials to the electrolyte which is ionically bridged. The ions are allowed to flow between the two solutions created when the two metals contact the electrolyte; the reaction difference of the two metals generates electricity. The difference between the two types of cells is that a galvanic cell must use dissimilar metals which are separated, except for ions, to produce a charge whereas an electrolytic cell has both anode and cathode suspended in the same solution and is driven by an external electrical charge; further, an electrolytic cell may use the same metal for cathode and anode.

Anode and cathode marking compared to charging

The anode and cathode in both types of cells are marked with the polarities of the current flow. In actual practice, the anode and the cathode in an electrolytic cell swap functions during the charge portion of the cycle (when acting as an electrolytic cell). Thus the electrode marked as anode for discharge is really acting as the cathode while charging and the electrode marked as cathode is actually acting as the anode during charging. In a galvanic cell, the anode is where the electrons come up from the solution and the oxidation reaction creates electrons from reaction with the negative anions. The cathode reduces the ionic solution, drawing positive cations to the cathode and using electrons to reduce the cation.

Usage

The electrolysis of salt water or acidic water is an easy example of electrolysis. The ionic solution is driven by current and produces hydrogen gas in a reduction reaction at the cathode using electrons to complete the hydrogen ions. At the anode oxygen gas is produced in an oxidizing reaction and electrons are given off as the oxygen ions combine. These electrons then flow up the anode and through the circuit.

In molten sodium chloride, when a current is passed through the salt the anode oxidizes chlorine which gives off electrons to the circuit. The cathode reduces sodium metal which deposits on the cathode using electrons to complete the sodium metal valence shell.

Commercially, electrolytic cells are used in electrorefining and electrowinning of several non-ferrous metals. Almost all high-purity copper, zinc and lead is produced industrially in electrolytic cells.

Cell types

 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Electrolytic_cell". A list of authors is available in Wikipedia.
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