Question

The substance which gets reduced acts as an oxidising agent.

• A. True
• B. False

Answer 1

The correct option is A True

Redox reaction: Reaction in which oxidation and reduction take place simultaneously.

• Oxidation means the loss of electrons, in this oxidation state increases.
• Reduction means the gain of electrons, in this oxidation state decreases.
• The one who gets oxidised acts as a reducing agent and the one who gets reduced acts as an oxidising agent.
• Example:

$2{\mathrm{FeCl}}_3\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)\to 2{\mathrm{FeCl}}_2\left(\mathrm{aq}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)+\mathrm{S}\left(\mathrm{s}\right)$
(Ferric chloride) (Hydrogen sulphide) (Ferrous chloride) (Hydrochloric acid) (Sulphur)

⦁ Here oxidation state of $\mathrm{S}$ in ${\mathrm{H}}_2\mathrm{S}$ is $-2$ and that of $\mathrm{Fe}$ in ${\mathrm{FeCl}}_3$ is $+3$ at the reactant side but the oxidation state of $\mathrm{S}$ in $\mathrm{S}$is $0$ and that of $\mathrm{Fe}$ in ${\mathrm{FeCl}}_2$ is $+2$ at the product side.
⦁ So, we can say that ${\mathrm{H}}_2\mathrm{S}$ is getting oxidised since its oxidation number is increasing from $-2$ to $0$ and ${\mathrm{FeCl}}_3$ is getting reduced since its oxidation number is decreasing from $+3$ to $+2$.
⦁ The one who gets oxidised acts as a reducing agent and the one who gets reduced acts as an oxidising agent.
⦁ So here ${\mathrm{H}}_2\mathrm{S}$ is a reducing agent and ${\mathrm{FeCl}}_3$is an oxidising agent.

Thus, the above statement is true.