(D) $1$. During the electrolysis of molten $NaCl$, the dissociation reaction is: $2NaCl(l) \rightarrow 2Na^+(l) + 2Cl^-(l)$.$2$. At the anode (oxidati

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(D) $1$. During the electrolysis of molten $NaCl$, the dissociation reaction is: $2NaCl(l) \rightarrow 2Na^+(l) + 2Cl^-(l)$.$2$. At the anode (oxidation): $2Cl^-(l) \rightarrow Cl_2(g) + 2e^-$. Pale green $Cl_2$ gas is evolved.$3$. At the cathode (reduction): $2Na^+(l) + 2e^- \rightarrow 2Na(l)$. Molten silvery-white sodium metal is deposited.$4$. Since both statements $A$ and $B$ are correct, the correct option is $D$.

Class 12 Chemistry Electrochemistry Electrolytes and Electrolysis

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Which of the following statements is correct regarding the electrolysis of molten $NaCl$?

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A
Pale green $Cl_2$ gas is released at the anode
B
Molten silvery-white sodium metal is deposited at the cathode
C
Decomposition of $NaCl$ into $Na$ metal and $Cl_2$ gas
D
Both options $A$ and $B$

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Which of the following statements is correct regarding the electrolysis of molten $NaCl$?

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Name the processes from which chlorine is obtained as a by-product. What will happen if an aqueous solution of $NaCl$ is subjected to electrolysis?

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Write the reactions for the following processes:
$A$. Electrolysis of water at the anode and cathode.
$B$. Electrolytic reaction of molten $NaCl$.