A device that uses electricity from an external source to drive a redox reaction.
an electrochemical cell used to cause a chemical change through the application of electrical energy; a cell in which electrolysis is taking place. (see voltaic cell)
A device, identical in constrution to the galvanic cell, in which the reverse of the thermodynamically spontaneous redox reaction is forced to occur by the application of a voltage in the opposite sense. The applied voltage must be greater than that produced by the corresponding galvanic cell. As in the galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode. However, the polarities are reversed in the electrolytic cell such that the anode is positive and the cathode is negative. Contrast with: Galvanic cell
An electrochemical cell in which electrolysis is done.
a cell containing an electrolyte in which an applied voltage causes a reaction to occur that would not occur otherwise (such as the breakdown of water into hydrogen and oxygen)
a cell in which current flows, power is consumed, and the cell reaction being driven is the reverse of the spontaneous cell reaction
Electrochemical battery that consume electricity.
a cell that uses electrical energy to produce a chemical change that would not otherwise occur.
An assembly, consisting of a vessel, electrodes, and an electrolyte, in which electrolysis can be carried out.
A device in which the chemical decomposition of material causes an electric current to flow. Also, a device in which a chemical reaction occurs as a result of the flow of electric current.
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.