Which is the best description of the behaviour of bromine in the reaction given below
`H_(2)O+Br_(2) rarr HOBr+HBr`

Options

A. Oxidised only
B. Reduced only
C. Proton acceptor only
D. Both oxidised and reduced

Answer

D

Explanation

`H_2O+underset(0)(Br_2)rarrunderset(+1)(HOBr)+underset(-1)(HBr)`
In the above reaction the oxidation number of `Br_2` increases from zero (in `Br_2` ) to +1 (in HOBr ) and decrease from zero ( `Br_2` ) to - 1 (in HBr ). Thus `Br_2` is oxidised as well as reduced & hence it is a redox reaction.