Question

Electrolysis of molten NaCl gives ____.
A. Na and ${H_2}$
B. Na and ${O_2}$
C. ${H_2}$ and ${O_2}$
D. Na and $C{l_2}$

Answer 1

Hint:Electrolysis is done for both the aqueous salt and molten salt. The product formed in both the electrolysis process is different. Electrolysis of a molten salt results in the production of elements from its own salt.

Complete answer:
The electrolysis is a process used to carry out a non-spontaneous chemical reaction under the influence of external current.
In electrolysis of molten sodium chloride, sodium chloride is melted at temperature above $801^\circ C$. The two electrodes one anode and one cathode is inserted to the molten state of sodium chloride and external electric current is passed through the molten sodium chloride salt. The chemical reaction takes place between the two electrodes.
The electrolysis cell used for molten sodium chloride salt is a commercial cell used for generating the sodium metal and chlorine gas from the molten salt of sodium chloride.
The liquid sodium melts at the cathode and is further drained off in the storage tank and the chlorine gas comes out from the molten state in the form of bubbles at anode.
The sodium ions move to the cathode where they gain electrons to form sodium metal.
The reaction is shown below.
$N{a^ + }(aq) + {e^ - } \to Na(s)$
The chloride ions move towards the anode, they release their electrons and get converted to chlorine gas.
$C{l^ - }(aq) \to \dfrac{1}{2}C{l_2}(g) + {e^ - }$
The overall reaction is given as shown below.
$2NaCl \to 2Na(s) + C{l_2}(g)$
Therefore, the correct option is D.

Note: In anode of electrochemical cell oxidation reaction takes place and in cathode of electrochemical cell reduction reaction takes place. It is a type of redox reaction.