Difference between Galvanic Cell and Electrolytic Cell
Galvanic Cells and Electrolytic Cells are both electrochemical cells and the major difference between them is as follows:
Galvanic Cell |
Electrolytic Cell |
---|---|
It converts chemical energy into electrical energy. | It converts electrical energy into chemical energy. |
The reactions are spontaneous in Galvanic Cell | The reactions are non-spontaneous in Electrolytic Cell. |
Both electrodes, cathodes, and anodes are placed in separate beakers | Both electrodes, cathodes, and anodes are placed in the same beaker. |
The electrolytes taken in both beakers are different. | Only one electrolyte is taken. |
Oxidation takes place at the anode (negative end), and reduction takes place at the cathode (positive end). | Oxidation takes place at the cathode (positive end), and reduction takes place at the anode (negative end). |
A salt bridge is used. | No salt bridge is used. |
Gibb’s free energy change during the reaction is negative. | Gibb’s free energy change during the reaction is positive. |
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Galvanic Cell
Galvanic Cell also called Voltaic Cell is an electrochemical device that converts spontaneous chemical energy generated in a redox reaction into electrical energy.
Table of Content
- What is Galvanic Cell?
- Cell Definition
- Electrolytic Cell Definition
- Electrochemical Cell Definition
- Primary Cell & Secondary Cell
- What is a Galvanic Cell?
- Parts of Galvanic Cell
- Constructions of Galvanic Cell
- Principle and Working of Galvanic Cell
- Electrode Potential
- Standard Electrode Potential
- Cell Potential
- Example of Galvanic Cell
- What is Salt Bridge?
- Difference between Galvanic Cell and Electrolytic Cell
- Solved Examples on Galvanic Cells