Question

In the electrolysis of molten copper chloride, the substance liberated at the anode is
(A) copper
(B) chlorine
(C) hydrogen
(D) copper chloride
(E) none of the above

Answer 1

Hint: Each electrode attracts ions that are of the opposite charge. Positively charged ions (cations) move towards the electron-providing (negative) cathode. Negatively charged ions (anions) move towards the electron-extracting (positive) anode.

Complete step by step answer:
Electrolysis is a technique that uses direct electric current (DC) to drive an otherwise non-spontaneous chemical reaction. Electrolysis is commercially important as a stage in the separation of elements from naturally occurring sources such as ores using an electrolytic cell. The voltage that is needed for electrolysis to occur is called the decomposition potential.
The quantity of the products is proportional to the current, and when two or more electrolytic cells are connected in series to the same power source, the products produced in the cells are proportional to their equivalent weight. These are known as Faraday's laws of electrolysis.
In the electrolysis of molten copper chloride, the substance liberated at the anode is chlorine and the substance deposited at cathode is copper.

Oxidation at anode:
     \[2C{{l}^{-}}\left( aq \right)\to C{{l}_{2}}\left( g \right)+2{{e}^{-}}\]
 Reduction at cathode:
     \[C{{u}^{2+}}\left( aq \right)+2{{e}^{-}}\to Cu\left( s \right)\]
So, the correct answer is “Option B”.

Note: Faraday's law of electrolysis: The laws state that (1) the amount of chemical change produced by current at an electrode-electrolyte boundary is proportional to the quantity of electricity used, and (2) the amounts of chemical changes produced by the same quantity of electricity in different substances are proportional to their equivalent weights.