Electrolytic Cell V/s Galvanic Cell
The main points of difference between an electrolytic cell and a galvanic cell (electrochemical cell) are:
Difference between an electrolytic cell and a galvanic cell
Electrochemical cell (Galvanic Cell) | Electrolytic cell |
---|---|
A Galvanic cell converts chemical energy into electrical energy. | An electrolytic cell converts electrical energy into chemical energy. |
Here, the redox reaction is spontaneous and is responsible for the production of electrical energy. | The redox reaction is not spontaneous and electrical energy has to be supplied to initiate the reaction. |
The two half-cells are set up in different containers, being connected through the salt bridge or porous partition. | Both the electrodes are placed in a same container in the solution of molten electrolyte. |
Here the anode is negative and cathode is the positive electrode. The reaction at the anode is oxidation and that at the cathode is reduction. | Here, the anode is positive and cathode is the negative electrode. The reaction at the anode is oxidation and that at the cathode is reduction. |
The electrons are supplied by the species getting oxidized. They move from anode to the cathode in the external circuit. | The external battery supplies the electrons. They enter through the cathode and come out through the anode. |
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ReplyDeletecell with a Cu and Ag electrode in their respective salt solutions
ReplyDeleteIs this a galvanic or electrolytic cell? Which electrode gets etched and which one will get deposition?
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ReplyDeletePlz replace the 'electrochemical cell' by 'voltaic cell'.....bcoz electrolytic n galvanic cells come under the category of electrochemical cells....
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