2nd November 2019


What is the difference between a galvanic cell and an electrolytic cell?

A galvanic cell transforms the energy released by a spontaneous redox reaction into electrical energy that can be used to perform work. An electrolytic cell converts electrical energy into chemical energy. Here, the redox reaction is spontaneous and is responsible for the production of electrical energy.

Furthermore, what is electrolytic cell and electrochemical cell?

An electrolytic cell is an electrochemical cell that drives a non-spontaneous redox reaction through the application of electrical energy. They are often used to decompose chemical compounds, in a process called electrolysis—the Greek word lysis means to break up.

How is an electrolytic cell different from a voltaic cell?

Electrolytic cells are very similar to voltaic (galvanic) cells in the sense that both require a salt bridge, both have a cathode and anode side, and both have a consistent flow of electrons from the anode to the cathode. However, there are also striking differences between the two cells.

What is an electrochemical cell?

The electrochemical cells which generate an electric current are called voltaic cells or galvanic cells and the other ones are called electrolytic cells which are used to drive chemical reactions like electrolysis. A common example of an galvanic cells is a standard 1.5 - volt cell meant for consumer use.
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