Electrolytic cell: Difference between revisions
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{{Short description|Device that uses electrical energy to drive a non-spontaneous chemical reaction}} | {{Short description|Device that uses electrical energy to drive a non-spontaneous chemical reaction}} | ||
[[File:Electrolyser 1884.png|Electrolyser 1884|thumb]] | |||
An '''electrolytic cell''' is a type of [[electrochemical cell]] that uses electrical energy to drive a non-spontaneous [[chemical reaction]]. This process is known as [[electrolysis]]. Electrolytic cells are used in various industrial applications, including the extraction of metals from their ores, electroplating, and the production of chemicals. | An '''electrolytic cell''' is a type of [[electrochemical cell]] that uses electrical energy to drive a non-spontaneous [[chemical reaction]]. This process is known as [[electrolysis]]. Electrolytic cells are used in various industrial applications, including the extraction of metals from their ores, electroplating, and the production of chemicals. | ||
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== Components == | == Components == | ||
An electrolytic cell consists of three main components: | An electrolytic cell consists of three main components: | ||
* | * '''Electrolyte''': A substance containing free [[ions]] that carry electric current. The electrolyte can be a [[molten]] ionic compound or an [[aqueous solution]]. | ||
* | * '''Anode''': The electrode where [[oxidation]] occurs. In an electrolytic cell, the anode is connected to the positive terminal of the power supply. | ||
* | * '''Cathode''': The electrode where [[reduction]] occurs. The cathode is connected to the negative terminal of the power supply. | ||
== Working Principle == | == Working Principle == | ||
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== Applications == | == Applications == | ||
Electrolytic cells have a wide range of applications, including: | Electrolytic cells have a wide range of applications, including: | ||
* | * '''[[Electroplating]]''': The process of depositing a thin layer of metal onto the surface of another material. This is commonly used to improve corrosion resistance, reduce friction, or enhance appearance. | ||
* | * '''[[Electrorefining]]''': The purification of metals by electrolysis. For example, copper is purified using an electrolytic cell. | ||
* | * '''[[Electrolysis of water]]''': The decomposition of water into oxygen and hydrogen gas. This process is used to produce hydrogen fuel. | ||
* | * '''[[Chlor-alkali process]]''': The production of chlorine and sodium hydroxide by the electrolysis of brine (sodium chloride solution). | ||
== Examples == | == Examples == | ||
Some common examples of electrolytic cells include: | Some common examples of electrolytic cells include: | ||
* | * '''[[Downs cell]]''': Used for the production of metallic sodium and chlorine gas from molten sodium chloride. | ||
* | * '''[[Hall-Héroult process]]''': Used for the extraction of aluminum from its ore, bauxite, through the electrolysis of molten aluminum oxide. | ||
== See also == | == See also == | ||
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[[Category:Chemical engineering]] | [[Category:Chemical engineering]] | ||
{{Electrolysis}} | {{Electrolysis}} | ||
{{ | {{chemistry-stub}} | ||
Latest revision as of 17:51, 3 March 2025
Device that uses electrical energy to drive a non-spontaneous chemical reaction
An electrolytic cell is a type of electrochemical cell that uses electrical energy to drive a non-spontaneous chemical reaction. This process is known as electrolysis. Electrolytic cells are used in various industrial applications, including the extraction of metals from their ores, electroplating, and the production of chemicals.
Components[edit]
An electrolytic cell consists of three main components:
- Electrolyte: A substance containing free ions that carry electric current. The electrolyte can be a molten ionic compound or an aqueous solution.
- Anode: The electrode where oxidation occurs. In an electrolytic cell, the anode is connected to the positive terminal of the power supply.
- Cathode: The electrode where reduction occurs. The cathode is connected to the negative terminal of the power supply.
Working Principle[edit]
When an external electric current is applied to the electrolytic cell, it forces the non-spontaneous chemical reaction to occur. The power supply provides the necessary energy to drive the reaction. At the anode, oxidation takes place, releasing electrons into the external circuit. At the cathode, reduction occurs, consuming electrons from the external circuit.
Applications[edit]
Electrolytic cells have a wide range of applications, including:
- Electroplating: The process of depositing a thin layer of metal onto the surface of another material. This is commonly used to improve corrosion resistance, reduce friction, or enhance appearance.
- Electrorefining: The purification of metals by electrolysis. For example, copper is purified using an electrolytic cell.
- Electrolysis of water: The decomposition of water into oxygen and hydrogen gas. This process is used to produce hydrogen fuel.
- Chlor-alkali process: The production of chlorine and sodium hydroxide by the electrolysis of brine (sodium chloride solution).
Examples[edit]
Some common examples of electrolytic cells include:
- Downs cell: Used for the production of metallic sodium and chlorine gas from molten sodium chloride.
- Hall-Héroult process: Used for the extraction of aluminum from its ore, bauxite, through the electrolysis of molten aluminum oxide.
See also[edit]
References[edit]
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| Articles related to electrolysis / Standard electrode potential | ||||||
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