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 $$ 2 \mathrm{NaCl} \longrightarrow 2 \mathrm{Na}(\mathrm{s})+\mathrm{Cl}_2 \text { (g) } $$