Question

In The Reaction Of $\mathrm{Zn}+{\mathrm{FeSO}}_4\to {\mathrm{ZnSO}}_4+\mathrm{Fe}$:

• A. $\mathrm{Fe}$ gets oxidized
• B. $\mathrm{Zn}$ gets oxidized
• C. $\mathrm{Zn}$ and $\mathrm{Fe}$ both get oxidized
• D. None of these

Answer 1

The correct option is B

$\mathrm{Zn}$ gets oxidized

The correct option is (B) :- $\mathrm{Zn}$ gets oxidized

The explanation for the correct answer:

Redox reactions:-

1. It is actually a type of chemical reaction in which the oxidation state of the substrate will change.
2. Oxidation is actually the loss of electrons which can also be depicted as the increase of the oxidation state of the chemical atoms.
3. The reduction is the gain of the electrons which can also be depicted as the decrease in the oxidation state of the chemical atoms.
4. If there is an increase in the oxidation number, it will describe the oxidation reaction.
5. So, according to the reaction $\underset{\mathrm{Zinc}}{\mathrm{Zn}\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}\mathrm{sulfate}}{{\mathrm{FeSO}}_4\left(\mathrm{aq}\right)}\to \underset{\mathrm{Zinc}\mathrm{sulfate}}{{\mathrm{ZnSO}}_4\left(\mathrm{aq}\right)}+\underset{\mathrm{Iron}\mathrm{ppt}.}{\mathrm{Fe}\left(\mathrm{s}\right)}\downarrow$, $\mathrm{Zn}$ will get oxidized as the oxidation state of $\mathrm{Zn}$ will increase from 0 to +2 ( from the reactant side to the product side), and the oxidation state of $\mathrm{Fe}$ decreases from +2 to 0 (from the reactant side to the product side) which will show a reduction.
6. Therefore, the reaction $\mathrm{Zn}$ will get oxidized.

The explanation for the incorrect answers:

Option (A): $\mathrm{Fe}$ gets oxidized

1. The oxidation state of $\mathrm{Fe}$ is getting decreased from +2 to 0 (from the reactant side to the product side)
2. So, in the reaction $\underset{\mathrm{Zinc}}{\mathrm{Zn}\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}\mathrm{sulfate}}{{\mathrm{FeSO}}_4\left(\mathrm{aq}\right)}\to \underset{\mathrm{Zinc}\mathrm{sulfate}}{{\mathrm{ZnSO}}_4\left(\mathrm{aq}\right)}+\underset{\mathrm{Iron}\mathrm{ppt}.}{\mathrm{Fe}\left(\mathrm{s}\right)}\downarrow$; $\mathrm{Fe}$ gets reduced.

Option (C): $\mathrm{Zn}$ and $\mathrm{Fe}$ both get oxidized

1. In the reaction: $\underset{\mathrm{Zinc}}{\mathrm{Zn}\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}\mathrm{sulfate}}{{\mathrm{FeSO}}_4\left(\mathrm{aq}\right)}\to \underset{\mathrm{Zinc}\mathrm{sulfate}}{{\mathrm{ZnSO}}_4\left(\mathrm{aq}\right)}+\underset{\mathrm{Iron}\mathrm{ppt}.}{\mathrm{Fe}\left(\mathrm{s}\right)}\downarrow$ there is a decrease in the oxidation state of $\mathrm{Fe}$ and increase in the oxidation state of $\mathrm{Zn}$.
2. Therefore, only $\mathrm{Zn}$ gets oxidized.

Option (D): None of these

1. As in the reaction, the oxidation state of $\mathrm{Zn}$ is getting increased so it will get oxidized
2. And then, this option is practically wrong.

Hence, the correct option is (B):- $\mathrm{Zn}$ gets oxidized