Chemistry - Electrochemistry Question with Solution | TestHub

During the electrolysis of molten $\text{NaCl}$, the ions present are ${\text{Na}}^{+}$ and ${\text{Cl}}^{-}$.

At the cathode (reduction):
${\text{Na}}^{+}+e^{-}\to \text{Na}(l)$
Since the operating temperature is much higher than the melting point of sodium, molten silvery-white sodium metal is deposited at the cathode.

At the anode (oxidation):
$2{\text{Cl}}^{-}\to {\text{Cl}}_2(g)+2e^{-}$
Pale green chlorine gas is liberated at the anode.

Since both statements A and B correctly describe the observations at the respective electrodes during the electrolysis process, the correct choice is both A and B.

Answer: Both options A and B