The products of electrolysis of aqueous NaCl solution are

When aqueous solution of NaCl is electrolysed , the following reaction takes place. 

${\mathrm{NaCl}}_{\left(\mathrm{aq}\right)}\to {\mathrm{Na}}_{\left(\mathrm{aq}\right)}^{+\hspace{0.17em}}+\hspace{0.17em}\hspace{0.17em}{\mathrm{Cl}}_{\left(\mathrm{aq}\right)}^{-}+\hspace{0.17em}{\mathrm{H}}_{\left(\mathrm{aq}\right) }^{+\hspace{0.17em}}+\hspace{0.17em}{\mathrm{OH}}_{\left(\mathrm{aq}\right)}^{-}$

According to preferential discharge theory, H⁺ is discharged at cathode and Cl^- is discharged at anode. 

Anode: $2{\mathrm{Cl}}^{-}\to {\mathrm{Cl}}_2+\hspace{0.17em}2{\mathrm{e}}^{-}\left(\mathrm{oxidation}\right)$

Cathode : $2{\mathrm{H}}^{+}+\hspace{0.17em}2{\mathrm{e}}^{-}\to {\mathrm{H}}_2 (\mathrm{reduction} )\hspace{0.17em}$