Question

In the reaction:
$2{\mathrm{H}}_2\mathrm{S}+{\mathrm{SO}}_2\to 2{\mathrm{H}}_2\mathrm{O}+3\mathrm{S}$

Choose the statements which is/are false?

• A. ${\mathrm{H}}_2\mathrm{S}$ is oxidised.
• B. ${\mathrm{SO}}_2$ is reduced.
• C. ${\mathrm{H}}_2\mathrm{S}$ is reduced.
• D. All are false.

Answer 1

The correct option is C

${\mathrm{H}}_2\mathrm{S}$ is reduced.

The explanation for the correct option:

1. The oxidation reaction is a type of reaction in which an atom loses electrons and its oxidation state increases.
2. A reduction reaction is a type of reaction in which an atom gains electrons and its oxidation state decreases.

(C) ${\mathrm{H}}_2\mathrm{S}$ is reduced.

It is the only false statement because H₂S is getting oxidized.

The explanation for the incorrect option:

(A) ${\mathrm{H}}_2\mathrm{S}$ is oxidized

In the reaction given to us, the oxidation state of sulfur in H₂S goes from -2 to 0, hence it is oxidized.

${\mathrm{H}}_2\mathrm{S}\to \mathrm{S}+2{\mathrm{H}}^{+}+2{\mathrm{e}}^{-}$

(B) ${\mathrm{SO}}_2$ is reduced.

In sulfur dioxide$\left({\mathrm{SO}}_2\right)$, sulfur is reduced oxidation state changes from +4 to 0. So the given statement is also true.

${\mathrm{SO}}_2\to 2\mathrm{S}$

(D) All are false.

This statement is false because options (A) and (B) are correct.

Therefore, the correct option is (C).