Galvanic Cell V/S Electrolytic Cell

 

Difference Between Galvanic Cell and Electrolytic Cell

Sr. No.	Galvanic Cell	Electrolytic Cell
1	It is a cell that converts chemical energy into electrical energy.	It is a cell that converts electrical energy into chemical energy.
2	It works spontaneously, meaning the redox reaction occurs naturally.	It works non-spontaneously and requires an external power supply.
3	The anode is negative because it supplies electrons.	The anode is positive because it is connected to the positive terminal of the battery.
4	The cathode is positive because it receives electrons.	The cathode is negative because it is connected to the negative terminal of the battery.
5	Oxidation occurs at the anode and reduction at the cathode (same as electrolytic cell).	Oxidation occurs at the anode and reduction at the cathode (same as galvanic cell).
6	Used to generate electricity (e.g., dry cells, Daniell cell).	Used for chemical processes like electroplating, electrolysis of water, and extraction of metals.
7	No external power source is required.	An external power source is essential for operation.
8	Energy is released in the form of electricity.	Energy is consumed in the form of electricity.
9	Example: Daniell Cell, Dry Cell.	Example: Electroplating, Electrolysis of NaCl.

Conclusion:
Both galvanic and electrolytic cells involve redox reactions, but they work in opposite ways. The galvanic cell produces electrical energy from chemical reactions, while the electrolytic cell uses electrical energy to drive chemical reactions.