Question

Write the difference between electrolytic and galvanic cells?

Answer 1

Galvanic cells and electrolytic cells are the electrochemical cells. An electrochemical cell is basically a device which has the capability to generate electrical energy through the chemical reactions that occur in it or utilise the electrical energy that is supplied to it in order to facilitate the chemical reactions in it. These cells either convert chemical energy into electrical energy, or electrical energy into chemical energy.

Complete answer:
The difference between electrolytic and galvanic cells has been stated below in a tabulated form:

S. No.	Electrolytic cells	Galvanic cells
1.	In electrolytic cell electricity is consumed	In galvanic cell electricity is produced
2.	electrolytic cells usually involve the non-spontaneous reactions thus requiring an external electron source	Galvanic cells usually derive its energy from the spontaneous redox reactions
3.	In electrolytic cells these terms are change anode is negatively charged and cathode in positively charged terminals	In galvanic cell anode is positive terminal and cathode is negative terminal
4.	in electrolytic solutions the both electrodes are dipped in single solution containing container	In galvanic cell both electrodes are dipped in two different solutions
5.	Chemical reaction in electrolytic cell is electrolysis of water:$2{H_2}O \to 2{\text{ }}{H_2} + {O_2}$	In galvanic cell chemical reaction is:$C{u^{2 + }} + Z{n^{}} \to Z{n^{2 + }} + Cu$
6.	In electrolytic cell, electrical energy is converted into chemical energy	In galvanic cell, chemical energy is converted into electrical energy

Note: Galvanic cells can become electrolytic cells. Galvanic cells being spontaneous need to attain energy in order to get converted into the electrolytic cell. Moreover, the anode as well as the cathode of the galvanic cell are switched and thus, the reaction has to be performed in a reverse manner such that the galvanic cell is converted into the electrolytic cell.