In the electrolysis of molten NaCl, is deposited at the cathode, whereas in electrolysis of aq. NaCl, is produced at the cathode.

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O_{2}

gas

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H_{2}

gas

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Solution

The correct options are
A Na
D $H_{2}$ gas
Electrolysis of molten sodium chloride:
At anode (sodium metal gets deposited):
${Na}^{+} + e^{-} \to Na$
At cathode (chlorine gas is liberated):
$2 {Cl}^{-} \to {Cl}_{2} + 2 e^{-}$
Overall reaction:
$2 NaCl (s) \to 2 Na (s) + {Cl}_{2} (g)$

Electrolysis of aqueous solution of sodium chloride:
At anode (chlorine gas is liberated):
$2 {Cl}^{-} \to {Cl}_{2} + 2 e^{-}$
At cathode (hydrogen gas is liberated):
$H_{2} O + 2 e^{-} \to {H_{2}}_{2} + 2 {OH}^{-}$

Overall reaction:
$2 {NaCl (aq) + 2 H_{2} O (l) \to 2 {Na}^{+} (aq) + 2 {OH}^{-} (aq) + H_{2} (g) + {Cl}_{2} (g)}_{2}^{+}$

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Which of the following statements are correct?

a) The electrolysis of aqueous NaCl produces hydrogen gas at the cathode and chlorine gas at the anode .

b) The electrolysis of a $C u S O_{4}$ solution using Pt electrodes causes the liberation of $O_{2}$ at the anode and the deposition of copper at the cathode .

c) Oxygen and hydrogen are produced at the anode and cathode during the electrolysis of dilute aqueous solution of $H_{2} S O_{4}$ .

d) All electrolytic reactions are redox reactions .

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