An electrolytic cell is a device that uses electrical energy to drive a non-spontaneous chemical reaction. It is mainly used in the process of electrolysis.
Parts of an electrolytic cell:
- Electrolyte – A molten or aqueous ionic compound that conducts electricity.
- Electrodes – Two conductors placed in the electrolyte:
- Cathode (–): Negative electrode where reduction (gain of electrons) takes place.
- Anode (+): Positive electrode where oxidation (loss of electrons) takes place.
- Power Source – A battery or DC supply that pushes electrons through the electrodes.
How it works:
- The external power source forces ions to move.
- Cations (positive ions) move toward the cathode and gain electrons.
- Anions (negative ions) move toward the anode and lose electrons.
Example:
- In the electrolysis of molten NaCl, an electrolytic cell decomposes sodium chloride into:
- Sodium metal at the cathode.
- Chlorine gas at the anode.
In simple words: An electrolytic cell is a setup that uses electricity to break down compounds into their elements.