Difference between Galvanic Cell and Electrolytic Cell
The differences between Galvanic Cell and Electrolytic Cell are :
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Galvanic Cell / Voltaic Cell |
Electrolytic Cell |
|---|---|
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Galvanic Cell vs. Electrolytic Cell- Difference |
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| Chemical energy is turned into electrical energy in these electrochemical cells. | Electrical energy is turned into chemical energy in these cells. |
| The redox reactions that take place in these cells are completely random. | The redox reactions in these cells require energy input to continue, indicating that the reactions are not spontaneous. |
| The anode in these electrochemical cells is negatively charged, whereas the cathode is positively charged. | A positively charged anode and a negatively charged cathode are included in these cells. |
| The electrons are produced by the species that undergo oxidation. | Electrons come from somewhere else (such as a battery). |
| Two electrodes are set up in two different vessels. | Both electrodes are set up in the same vessel. |
Electrochemical Cells
Electrochemical Cell is a device that may either generate electrical energy from chemical reactions or use electrical energy that is supplied to it to speed up chemical reactions. There are various types of electrochemical cells and they are used in our daily activities such as cells that are used in Watches, TV remotes, Clocks, etc.
In this article, we will learn about the basic concepts and topics of electrochemical cell, its representation, diagram, working principle, structure and notation. We will also explore the parts, types, and applications of electrochemical cell, along with its difference from electrolytic cell in detail.
Table of Content
- What is an Electrochemical Cell?
- Half-Cells and Cell Potential
- Primary and Secondary Cells
- Electrochemical Cell Types
- Salt Bridge
- Electrochemical Cell and Electrolytic Cell- Difference