Explanation:

Electrolytic Cell

Definition of Galvanic and Electrolytic Cell

In galvanic cells there are spontaneous REDOX processes that allow continuous flow of electrons through the conductor, whereby the chemical energy is converted into electric. In an electrolytic cell, redox reactions take place under the INFLUENCE of an external source, where the electricity is converted into a chemical energy. The redox reactions are non-spontaneous.

Technique of Galvanic and Electrolytic Cell

Galvanic cells generate electricity with the aid of chemical reactions. In electrolytic cells, an electric current is used for development of a chemical reaction, utilizing an external source along the way.

Design of Galvanic and Electrolytic Cell

Galvanic cells consists of two different electrodes immersed in solutions of their ions that are separated by a semipermeable membrane or a salt bridge. Electrolytic cells consist of an electrolytic container in which two electrodes are connected to a DC source. The electrolyte may be a melt or an aqueous solution of some salt, acid or alkali.

Electrode polarity in Galvanic and Electrolytic Cell

In galvanic cells the anode is the negative and the cathode is the positive electrode. In electrolytic cells, the opposite occurs.

Chemical reaction in Galvanic and Electrolytic Cell

In case of galvanic cell, the oxidation reaction takes place at the anode (negative electrode) where there is a surplus of negative charge. At the cathode, the reduction reaction happens, inducing a positive BUILDUP of charge. In case of electrolytic cell an outside source is used to trigger a reaction. At the negative electrode, the electrons are pushed out of it – so the reduction phase will happen on the negative electrode. On the positive electrode the oxidation phase takes place – and this is the anode.

Application of Galvanic and Electrolytic Cell

Galvanic cells are used as a source of electrical current, and are more commonly referred to as batteries or accumulators. Electrolytic cells have different practical uses, some of them being making hydrogen and oxygen gas for commercial and industrial applications, electroplating, extracting pure METALS