Question

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

Answer 1

Hint:Zn is reacted with iron sulphate and forms zinc sulphate and iron. When zinc is added to the solution of iron sulphate, the color of iron sulphate solution changes. It happens because zinc is more reactive than iron, therefore it displaces iron from its iron sulphate solution and a grey precipitate of an iron and a colorless solution of zinc sulphate is formed.

Complete step by step answer:
Zinc added in the solution of iron sulphate, the color of sulphate solution becomes change and zinc is more reactive element than iron so it displaces iron from solution and forms precipitates of grey colored of iron and solution becomes colorless and formed zinc sulphate.
Here the chemical reaction is given below:
 $Zn - 2{e^ - } \to Z{n^{II}}(oxidation)$
 $F{e^{II}} + 2{e^ - } \to F{e^0}(\operatorname{Re} duction)$
As we see the above reaction, the oxidation number of zinc is 0 to +2. So, increasing the oxidation number describes that the reaction gets an oxidation reaction. From the above reaction, Zn gets oxidized and Fe shows the reduction reaction because an oxidation number decreases from +2 to 0.
So overall reaction given as below:
 $Zn + FeS{O_4} \to ZnS{O_4} + Fe:$
Where Zn gets oxidized.
Hence option (A) is the correct answer.

Note:This reaction is a redox reaction. Redox reaction contains both oxidation and reduction reactions. Here zn gets oxidized and reduces iron. A loss of negatively charged electrons corresponds to an increase in oxidation number, while a gain of electrons corresponds to a decrease in oxidation number. Therefore, the Zn is oxidized undergoes an increase in oxidation number and Fe is reduced undergoes a decrease in oxidation number.