Question

In the reaction of $Zn + FeS{O_4} \to ZnS{O_4} + Fe$ :
A. $Zn$ gets oxidised
B. $Fe$ gets oxidised
C. $Zn$ is oxidising agent
D. $Zn$ and $Fe$ both get oxidised

Answer 1

A reaction in which oxidation and reduction take place simultaneously is termed as a redox reaction . In the given reaction both oxidation and reduction take place . We have to find which element is oxidised and which is reduced .

Complete step by step answer:
Oxidation is the process of addition of oxygen atom or removal of hydrogen atom whereas reduction is the process of removal of oxygen or addition of oxygen atom.They occur in the presence of oxidising or reducing agents respectively. When both processes occur simultaneously in a reaction it is said to be a redox reaction.
The substance which is oxidised acts as the reducing agent while the substance reduced acts as the oxidising agent.
Oxidation is also said to occur when the oxidation state of an element increases.
Oxidation state is the total number of electrons that an atom loses or gains to form a bond with another atom.
Also, the oxidation state of an atom in its elemental form is always zero.
In the given reaction,
$Zn + FeS{O_4} \to ZnS{O_4} + Fe$
The oxidation state of $Zn$ increases from zero ( in elemental state ) to +2 (as in $ZnS{O_4}$ ) because it loses two electrons.
while the oxidation state of $Fe$ decreases from +2 ( in $FeS{O_4}$ ) to zero (in elemental state ) as it gains two electrons.
It is clear from above that $Zn$ gets oxidised to $ZnS{O_4}$ and $FeS{O_4}$ gets reduced to $Fe$ .

So, the correct answer is Option A .

Note:
The given reaction is also an example of metal displacement reaction . A metal displacement reaction is one in which a metal of one compound is replaced by some other metal of another compound . For example , in the given reaction $Fe$ is replaced by $Zn$ .