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Electrolysis of molten sodium chloride(nacl) redox reaction equations explaining Oxidation half and reduction half cell reactions in electrolytic cell:

What is Electrolysis?
Electrolysis is the decomposition of an electrolyte by the passage of electricity through molten or aqueous solution of the electrolyte.

What is Electrolyte?
A substance in aqueous or molten form dissociate into ions and can conduct heat
& electricity .
A source of direct current is connected to a pair of inert electrodes inserted in molten sodium chloride.
Na+ ions flows towards the negative & Cl ions towards the positive electrode.
Anode is +ve
Cathode is ve
Oxidation takes place at Anode
Reduction at Cathode.
Explanation of Electrolysis of NaCl (Electrolytic Cell Redox reaction):
Cl ions that collide with the positive electrode are oxidized to Cl2 gas, which bubbles off at anode.
At Anode(+ve electrode) Oxidation occurs

When Na+ ions collide with the negative electrode,The battery carries a large enough potential to force these ions to pick up electrons to form sodium metal
At Cathode( ve electrode) Reduction occurs.
The net effect of passing an electric current Through the molten NaCl in the cell decomposes it into its elements, Sodium metal & chlorine gas
All these points explained with 3d animation will clear the concept of electrolysis of nacl for Class 910 icse ,Class 1112 ,o/a levels Chemistry in Urdu or Hindi.

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