What are the two main types of electrochemical cells?

The two main types of electrochemical cells are galvanic and electrolytic cells. Galvanic cells, also known as voltaic cells, generate electrical energy from spontaneous chemical reactions, typically involving oxidation-reduction (redox) reactions. They convert chemical energy into electrical energy; a common example is a battery. In a galvanic cell, the flow of electrons occurs from the anode (where oxidation takes place) to the cathode (where reduction occurs) through an external circuit, generating an electric current.

On the other hand, electrolytic cells require an external source of electrical energy to drive a non-spontaneous chemical reaction. In these cells, electrical energy is converted back into chemical energy. This is often seen in processes like electroplating or the electrolysis of water, where electrical energy is used to split water into hydrogen and oxygen gases. In an electrolytic cell, the flow of electrons is reversed, with the anode being the site of oxidation and the cathode being the site of reduction, but in this case, it is driven by an external current.

Together, these two types represent the fundamental operations of electrochemical systems, encompassing both energy generation and energy consumption. Recognizing their distinct functions and principles is crucial for understanding various