Question

Which of the following compounds is formed when $FeS{{O}_{4}}$ reacts with an oxidizing agent?
(a)- FeS
(b)- FeO
(c)- $Fe{{(OH)}_{2}}$
(d)- $F{{e}_{2}}{{(S{{O}_{4}})}_{3}}$

Answer 1

Hint: When a compound is oxidized then the central atom of the compound changes its oxidation state, i.e., there will be an increase in the oxidation number. So, the given compound is $FeS{{O}_{4}}$ and the oxidation number of iron in it is +2.

Complete answer:
Oxidation and reduction reactions are common reactions taking place in chemistry. When the compound is oxidized or reduced its properties change.
 When a compound is oxidized then the central atom of the compound changes its oxidation state, i.e., there will be an increase in the oxidation number. When a compound is reduced then the central atom of the compound changes its oxidation state, i.e., there will be a decrease in the oxidation number.
The given compound in the question is $FeS{{O}_{4}}$ and it is reacting with an oxidizing agent so, the product the oxidation number of iron will increase.
The oxidation number of iron in $FeS{{O}_{4}}$ is +2.
In the given compounds in the options, the oxidation number of iron are:
(a)- FeS
In this, the oxidation number will be +2.
(b)- FeO
In this, the oxidation number will be +2.
(c)- $Fe{{(OH)}_{2}}$
In this, the oxidation number will be +2.
(d)- $F{{e}_{2}}{{(S{{O}_{4}})}_{3}}$
In this, the oxidation number will be +3.
So, the product formed will be $F{{e}_{2}}{{(S{{O}_{4}})}_{3}}$.

Therefore, the correct answer is option (d)- $F{{e}_{2}}{{(S{{O}_{4}})}_{3}}$

Note:
An example of reaction of $FeS{{O}_{4}}$ with an oxidizing agent like hydrogen peroxide in the presence of sulfuric acid. The reaction is given below:
$2FeS{{O}_{4}}+{{H}_{2}}S{{O}_{4}}+{{H}_{2}}{{O}_{2}}\to F{{e}_{2}}{{(S{{O}_{4}})}_{3}}+2{{H}_{2}}O$