Question

Identify oxidation and reduction with their agents.
$2Al + F{e_2}{O_3} \to 2Fe + A{l_2}{O_3}$

Answer 1

The redox reaction is a chemical reaction in which oxidation of reduction of reactants takes place simultaneously. During oxidation, electrons are lost during the reaction, so an increase in the oxidation number is observed whereas during reduction, electrons are gained during the reaction. Thus, the oxidation number is decreased.

Complete answer:
The given reaction proceeds as follows:
$2Al + F{e_2}{O_3} \to 2Fe + A{l_2}{O_3}$
In the reaction, the reduction and oxidation take place simultaneously, so it is a redox reaction. For better understanding of oxidation and reduction of reactants in the reaction, we need to write the half-reactions for it.
Half reactions: It is a part of the overall reaction which represents it in two parts i.e., oxidation half reaction and reduction half reaction. For the given redox equation, half cell reactions are as follows:
Oxidation half reaction: $A{l^{(0)}} \to A{l^{3 + }}$
As the oxidation state of aluminium increases from $0$ to $+ 3$. Therefore, we can say that $Al$ is oxidized to $A{l_2}{O_3}$.
Reduction half reaction: $F{e^{3 + }} \to F{e^{(0)}}$
As the oxidation state of iron decreases from $+ 3$ to $0$. Therefore, we can say that $F{e_2}{O_3}$ is reduced to $Fe$.
Oxidizing agent: It is also known as oxidant. It is a compound which itself gets reduced to oxidize other reactants in the reaction. In simple words we can say that, the reactant which is reduced during a reaction is known as oxidizing agent.
For the given reaction, $F{e_2}{O_3}$ is reduced. Therefore, the oxidizing agent is ferric oxide i.e., $F{e_2}{O_3}$.
Reducing agent: It is a compound which itself gets oxidized to reduce other reactants in the reaction. In simple words we can say that the reactant which is oxidized during a reaction is known as a reducing agent.
For the given reaction, $Al$ is oxidized. Therefore, the reducing agent is aluminium i.e., $Al$.

Note:
Before identifying oxidizing and reducing agents, make sure that the given redox reaction is balanced i.e., the number of atoms of each element should be equal to the number of atoms of each element in the product. Charge on the reactant and product side should also be balanced.