Question

In electrolysis of aqueous $NaCl,$ what volume of $C{{l}_{2\left( g \right)}}$ is produced in the time that it takes to liberate $5.0$ litre of ${{H}_{2\left( g \right)}}$ ? Assume that both gases are measured at STP.
(A) $5.0$
(B) $2.50$
(C) $7.50$
(D) $10.0$

Answer 1

Hint : We know that the electrolytic cell is a device that utilizes electrical energy to decompose some chemical compounds by a process known as Electrolysis. The electrolytic cell is nothing but a special kind of electrochemical cell. Electrolytic cells are those which work on the chemical energy by utilizing electrical power from the system.

Complete Step By Step Answer:
Electrochemical cells are devices based on the principle that when a chemical oxidation-reduction reaction occurs, electrons are being transferred from one chemical species to another. In a galvanic cell, the electrons are usually allowed to flow through outside of the device in a circuit to operate some electrical device. In the other type of electrochemical cell, called an electrolytic cell, the reverse process occurs. Electrons in the form of an electric current are deliberately being pumped through the chemicals in the section to force an electric current oxidation reduction reaction to take place. An example of an electrolytic cell is the setup used to decompose water into hydrogen and oxygen by electrolysis.
Electrolytic cells are those which work on the chemical energy by utilizing electrical power from the system. The electrolytic cells work on a similar mechanism as that of the Galvanic cells. Both the cells mainly consist of two half cells, such as the oxidation half-cell and redox half-cell. The overall reaction during the electrolysis of aqueous sodium chloride:
$2NaC{{l}_{\left( aq \right)}}+2{{H}_{2}}{{O}_{\left( l \right)}}\to 2Na_{\left( aq \right)}^{+}+2OH_{\left( aq \right)}^{-}+C{{l}_{2\left( g \right)}}+{{H}_{2\left( g \right)}}.$
It can be easily taken into consideration that one volume of hydrogen to one volume of chlorine is collected in the electrolysis. Number of equivalent of ${{H}_{2}}=$ Number of Equivalent of $C{{l}_{2}}$
Therefore, the correct answer is option A.

Note :
Remember that the electrolytic cells are very similar to voltaic (galvanic) cells because both require a salt bridge, both have a cathode and anode side, and both have a consistent flow of electrons from the anode to the cathode. However, there are also striking differences between the two cells.