Question

In the following reaction, identify the oxidized species, reduced species, oxidizing agent, and reducing agent. Be sure to answer all parts. Cl2(aq) + 2 KI(aq) → 2 KCl(aq) +12(aq) Cl, is the (select) KI is the (select) and the (select) and the (select) A. A.

Answer 1

`Cl_2` is reduced species.

`KI` is oxidized species.

`Cl_2` is oxidizing agent.

`KI` 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 :

`Cl_2(aq)+2KI(aq)\rightarrow 2KCl(aq)+I_2(aq)`

The half oxidation-reduction reactions are:

Oxidation reaction :
`2I^-\rightarrow I_2+2e^-`

Reduction reaction :
`Cl_2^++2e^-\rightarrow 2Cl^-`

From this we conclude that the
`'KI'` is the reducing agent that loses an electron to another chemical species in a redox chemical reaction and itself gets oxidized and
`'Cl_2'` is the oxidizing agent that gain an electron to another chemical species in a redox chemical reaction and itself gets reduced.

Thus,
`Cl_2` is reduced species.

`KI` is oxidized species.

`Cl_2` is oxidizing agent.

`KI` is reducing agent.