Answer :
Answer :
[tex]Cl_2[/tex] is reduced species.
[tex]KI[/tex] is oxidized species.
[tex]Cl_2[/tex] is oxidizing agent.
[tex]KI[/tex] is reducing agent.
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 balanced redox reaction is :
[tex]Cl_2(aq)+2KI(aq)\rightarrow 2KCl(aq)+I_2(aq)[/tex]
The half oxidation-reduction reactions are:
Oxidation reaction : [tex]2I^-\rightarrow I_2+2e^-[/tex]
Reduction reaction : [tex]Cl_2^++2e^-\rightarrow 2Cl^-[/tex]
From this we conclude that the [tex]'KI'[/tex] is the reducing agent that loses an electron to another chemical species in a redox chemical reaction and itself gets oxidized and [tex]'Cl_2'[/tex] is the oxidizing agent that gain an electron to another chemical species in a redox chemical reaction and itself gets reduced.
Thus, [tex]Cl_2[/tex] is reduced species.
[tex]KI[/tex] is oxidized species.
[tex]Cl_2[/tex] is oxidizing agent.
[tex]KI[/tex] is reducing agent.