What is Electrolytic Cell?
Electrolysis is the procedure of decomposition of an electrolyte by the passage of electricity throughout its aqueous solution or the molten state of an electric current. This cell is utilized to perform electrolysis which is electrolyte cells.
Water, for example, can be electrolyzed (with the help of an electrolytic cell) to produce gaseous oxygen and hydrogen. This is accomplished by utilising the flow of electrons (into the reaction environment) to overcome the non-spontaneous redox reaction’s activation energy barrier.
The following are the three major components of electrolytic cells:
- Cathode: It is negatively charged for electrolytic cells
- Anode: It is a type of electrode that is (which is positively charged for electrolytic cells)
- Electrolyte: The electrolyte serves as a conduit for electrons to flow between the cathode and the anode. Water (containing dissolved ions) and molten sodium chloride are common electrolytes in electrolytic cells.
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Electrolysis
Electrolysis is the process of decomposing the ionic compound into its constituent elements by passing the electric current into the solution of the ionic compound. The concept of electrolysis was first given by the famous scientist of the 19th century Michael Faraday. It is a chemical process that uses electrical energy to bring changes in the chemical reaction. Electrolysis is used to separate components of the ionic compounds.
In this article, we will learn about, electrolysis, its process, faraday’s law of electrolysis and others in detail in this article.