Question

Name the chemical reaction. $Fe\; + \;CuS{O_4}\left( {aq.} \right)\; \to \;FeS{O_4}\left( {aq.} \right)\; + \;Cu\left( {\text{s}} \right)$

Answer 1

Hint : In above reaction Iron is reacting with aqueous Copper sulphate to form aqueous Ferrous sulphate and Copper. We will see this reaction and understand the process behind it to know the nature of the reaction.

Complete Step By Step Answer:
Redox reaction: It is defined as any reaction which involves change in oxidation number of an atom, ion, or molecule by gaining or losing an electron. It is also said to be an oxidation-reduction reaction because while an atom, ion, or molecule is oxidised another atom, ion, or molecule is reduced.
If we see the given reaction carefully, we will observe that Iron is oxidised and Copper is reduced. This can be observed from the following reaction
$Fe\; + \;C{u^{2 + }}\;\; \to \;\;F{e^{2 + }}\; + \;Cu$
We can see that the oxidation state of Iron is initially zero but after reaction it becomes two. On the other hand copper has an oxidation state equal to two initially but it is reduced to zero after the reaction.
Above reaction also can be termed as displacement reaction as iron is replacing copper ions from the aqueous copper sulphate solution. It is a single displacement reaction of one metal atom by another metal atom. As iron is placed above copper in reactivity series and elements which are above in reactivity series are more reactive so iron is more reactive than copper. The metallic iron is oxidised to Ferrous ion and Cupric ion is reduced to metallic Copper.

Note :
During this reaction the colour of the aqueous copper sulphate solution will change from blue to green-blue colour due to ferrous sulphate solution and copper metal is deposited as a red-brown precipitate.