During the electrolysis of fused \(\mathrm{NaCl}\), the product obtained at anode is

Anode: The electrode of an electrochemical cell at which oxidation occurs.
Cathode: The electrode of an electrochemical cell at which reduction occurs.
Electrolysis of molten \(\mathrm{NaCl}\) or fused \(\mathrm{NaCl}\)
Sodium ions migrate to cathode, where electron enter, the melt is reduced to sodium metal
\(
\mathrm{Na}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Cl}_2+\mathrm{e}^{-}
\)
Chlorine ions migrate to anode. They give up their electrons to the anode
and are oxidized to chlorine gas:
\(
\mathrm{Cl}^{-} \longrightarrow \frac{1}{2} \mathrm{Cl}_2+\mathrm{e}^{-}
\)
Overall reaction
\(
2 \mathrm{NaCl} \longrightarrow 2 \mathrm{Na}(\mathrm{s})+\mathrm{Cl}_2 \text { (g) }
\)