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 Cl2 gas.
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.
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13 thoughts on “Sodium Chloride Electrolysis Half reactions | Oxidation and Reduction Half reactions”
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