Question

Classify the following reaction on the basis of energy change :

$2\mathrm{NaCl}\left(\mathrm{l}\right)\stackrel{\mathrm{Electric}\mathrm{current}}{\to }2\mathrm{Na}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Answer 1

$\underset{\mathrm{Sodium}\mathrm{chloride}}{2\mathrm{NaCl}\left(\mathrm{l}\right)}\stackrel{\mathrm{Electric}\mathrm{current}}{\to }\underset{\mathrm{Sodium}}{2\mathrm{Na}\left(\mathrm{s}\right)}+\underset{\mathrm{Chlorine}}{{\mathrm{Cl}}_2\left(\mathrm{g}\right)}$

Electrochemical reaction- An electrochemical reaction is a process in which electrons flow between a solid electrode and a substance, such as an electrolyte. This flow triggers an electric current through the electrodes, causing the reaction to liberate or absorb heat.

In the above question, an electric current is passed to decompose sodium chloride into sodium and chlorine gas.

Hence, the answer is an electrochemical reaction.