Question

The behaviour of Bromine in the reaction given below is:

H₂O + Br₂ → HOBr + HBr

1. Proton acceptor only
2. Both oxidized and reduced
3. Oxidized only
4. Reduced only

Answer 1

Correct Answer - Option 2 : Both oxidized and reduced

Concept:

Redox Reaction:

CuO + H2 → Cu + H2O

• Oxidation and reduction are opposite in nature and they always take place simultaneously.
• In a chemical reaction, when one substance is reduced, the other is oxidized.
• In the reaction, CuO + H2 → Cu + H2O Cu is reduced whereas Hydrogen is oxidized.
• The reactions in which oxidation and reduction take place simultaneously are called Redox- reactions.
• When the oxidation state of a substance goes higher, it is said to be oxidized.
• When the oxidation state of a substance goes lower, it is said to be reduced.

Explanation:

• The reaction given is:​

H2O + Br2 → HOBr + HBr

• In the given reaction, the Bromine atom is in oxidation state zero, since it is in an elemental state.
• After undergoing the redox reaction, it changes to HOBr, the oxidation state of Br in HOBr is +1.
• The oxidation state of Br in HBr is -1.
• Hence, Bromine's state is changing from 0 to +1 and -1, one to a higher oxidation state and the other to a lower oxidation state.

Br2 → HOBr is the oxidation reaction

Br2 → HBr is the reduction reaction.

Hence, Bromine is getting both oxidized and reduced in the given reaction.

• The reaction given is a disproportionation reaction.
• It is a type of reaction where a compound changes from an oxidation state to a lower as well as to a higher oxidation state.