Respuesta :
Answer : The oxidizing and reducing agents are, [tex]H_2O_2[/tex] and [tex]Fe^{2+}[/tex].
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:
[tex]2H^+(aq)+H_2O_2(aq)+2Fe^{2+}(aq)\rightarrow 2Fe^{3+}(aq)+2H_2O(l)[/tex]
The half oxidation-reduction reactions are:
Oxidation reaction : [tex]Fe^{2+}\rightarrow Fe^{3+}+1e^-[/tex]
Reduction reaction : [tex]O^-+1e^-\rightarrow O^{2-}[/tex]
The oxidation state of oxygen in [tex]H_2O_2[/tex] and [tex]H_2O[/tex] 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, '[tex]Fe^{2+}[/tex]' act as a reducing agent and '[tex]H_2O_2[/tex]' act as a oxidizing agent.
Thus, the oxidizing and reducing agents are, [tex]H_2O_2[/tex] and [tex]Fe^{2+}[/tex].
