Sodium Chloride Electrolysis Half reactions | Oxidation and Reduction Half reactions

Sodium Chloride Electrolysis:

Do you know👀

Electrolysis is the passage of direct electric current through an ionic substance that is either molten or in aqueous form.

Methods of electrolysis of sodium chloride:

Two methods are most commonly used for the electrolysis of NaCl.
1.Molten Sodium Chloride.
2.Aqueous Sodium Chloride.

Let’s talk about the electrolysis of molten NaCl:

If a sodium chloride is melted at (above 801 Celsius ) ,the two electrodes are inserted in it and the electric current is passed into the molten salt,then the redox reaction takes place at electrodes.

Electrolysis of NaCl (molten) Half Reactions:
Cl- ions that collide with the positive electrode are oxidized to
Cl2 gas, which bubbles off at anode.

At Anode(+ve electrode): Oxidation half reaction
 2Cl-(aq)   →    Cl2(g) + 2e-

👉Cl– ions( 8e- in valance shell) migrate towards the anode.
They give up the electrons to the anode and oxidized to Clgas.

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 half reaction
 2Na+(aq) + 2e-   →   2Na(s)    

👉Na+ ions( 8e- in valance shell after losing 1e-) migrate to the
 cathode where after gaining electron/s reduced to  Na metal.
  Electrolysis of NaCl:
 2NaCl (l)  →   2Na(s) + Cl2(g)

The net effect of passing an electric current through the molten NaCl in the cell decomposes it into its elements, Sodium metal & chlorine gas.
Watch  Electrolysis of molten NaCl on Youtube

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