Identify the reaction taking place at anode during electrolysis of molten $\mathrm{NaCl}$ ?

Identify the reaction taking place at anode during electrolysis of molten $\mathrm{NaCl}$ ?
  1. $2 \mathrm{OH}^{-} \rightarrow \mathrm{H}_2 \mathrm{O}+\frac{1}{2} \mathrm{O}_2+2 \mathrm{e}^{-}$
  2. $2 \mathrm{H}^{+} 2 \mathrm{e}^{-} \rightarrow \mathrm{H}_2$
  3. $\mathrm{Na}^{+}+\mathrm{le}^{-} \rightarrow \mathrm{Na}_{(\mathrm{s})}$
  4. $2 \mathrm{Cl}^{-} \rightarrow \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-}$

Solution

At anode oxidation takes place and $\mathrm{Cl}^{-}$ions get oxidized at anode, $2 \mathrm{Cl}^{-} \rightarrow \mathrm{Cl}_2+2 \mathrm{e}^{-}$

Asked in: MHT CET 2022 (07 Aug Shift 1)

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