Question

$H_{2}S\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)+S\left(s\right)$

The reaction is interpreted as:

• A. H₂S is getting oxidised and Cl₂ is getting reduced
• B. H₂S is getting reduced and Cl₂ is getting oxidised
• C. only H₂S is getting oxidised
• D. Both H₂S and Cl₂ are getting reduced

Answer 1

The correct option is A

H₂S is getting oxidised and Cl₂ is getting reduced

Redox reactions

Reaction between two or more reactants in which one reactants is oxidised and the other is reduced is called a redox reaction. The species oxidised and reduced can be identified by analyzing the oxidation state of the species in reactants and the products. The reactant that gets reduced is called the oxidising agent and the reactant that gets oxidised is called a reducing agent in redox reactions.

Reaction between Hydrogen sulphide and Chlorine

During a redox reaction, electrons are transferred between reactants. The species that loses an electrons and thus increase its oxidation state is oxidised. The species undergoing reducing accepts the electron and thus decreases its oxidation state.

The balanced equation for the reaction is:

$H_{2}S\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)+S\left(s\right)$

(Hydrogen (Chlorine) (Hydrochloric (Sulphur)

sulphide) acid)

In this reaction, the oxidation state of sulphur increases from -2 in Hydrogen sulphide (H₂S) to 0 in Sulphur (S). Therefore, Hydrogen sulpphide is oxidized in the reaction. Also, the oxidation state of chlorine decreases from 0 in Chlorine gas (Cl₂) to -1 in Hydrochloric acid (HCl). Therefore, Chlorine undergoes reduction in the reaction.

Therefore, Hydrogen sulphide undergoes undergoes oxidation and and Chlorine undergoes reduction. Option (A) is correct and option (B) is incorrect.

Since chlorine also undergoes reduction, option (C) is incorrect.

Option (D) is incorrect because Hydrogen sulphide is oxidised in the reaction.

Therefore, the correct option is (A) H₂S is getting oxidised and Cl₂ is getting reduced.