Why are different products obtained when molten $M g C l_{2}$ and aqueous $M g C l_{2}$ are electrolysed with inert electrodes?

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Solution

Step-1 In Molten $M g C l_{2}$ ions:
When molten Magnesium chloride $M g C l_{2}$ is electrolysed with inert electrolytes,
$M g^{2 +} + 2 e^{-} \to M g 2 C l^{-} \to C l_{2} + 2 e^{-}$
Step-2 In Aqueous $M g C l_{2}$ ions:
When aqueous Magnesium chloride $M g C l_{2}$ is electrolysed with inert electrolytes,
$2 H^{+} + 2 e^{-} \to H_{2} (P r e f e r e n t i a l l y d i s c h a r g e o f H^{+} o v e r M g^{2 +}) 2 C l^{-} \to C l_{2} + 2 e^{-}$
Step 3: Products obtained during electrolysis of molten $M g C l_{2}$ and aqueous $M g C l_{2}$ using inert electrode
Molten $M g C l_{2}$ gives ${Mg}^{2 +}$ ion during electrolysis at cathode and ${Cl}^{-}$ ion at anode.
Aqueous $M g C l_{2}$ gives Hydrogen gas at cathode and oxygen gas at anode.

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