Question

Identify the oxidizing and reducing agents in the following: 2H+(aq) + H2O2(aq) + 2Fe2+(aq) → 2Fe3+(aq) + 2H2O(l)

Answer 1

Answer :  The oxidizing and reducing agents are, $H_2O_2$ and $Fe^{2+}$.

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Reducing agent : It is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.

Oxidizing agent : It is defined as the agent which helps the other substance to oxidize and itself gets reduced. Thus, it will undergo reduction reaction.

The given redox reaction is:

$2H^+(aq)+H_2O_2(aq)+2Fe^{2+}(aq)\rightarrow 2Fe^{3+}(aq)+2H_2O(l)$

The half oxidation-reduction reactions are:

Oxidation reaction : $Fe^{2+}\rightarrow Fe^{3+}+1e^-$

Reduction reaction : $O^-+1e^-\rightarrow O^{2-}$

The oxidation state of oxygen in $H_2O_2$ and $H_2O$ is, (-1) and (-2) respectively.

In this reaction, 'Fe' is oxidized from oxidation (+2) to (+3) and 'O' is reduced from oxidation state (-1) to (-2). Hence, '$Fe^{2+}$' act as a reducing agent and '$H_2O_2$' act as a oxidizing agent.

Thus, the oxidizing and reducing agents are, $H_2O_2$ and $Fe^{2+}$.