Which substance/ion is oxidised and which substance/ion is reduced in the following reaction?
$3 N_{2} H_{4} + 2 B r O_{3}^{-} \to 3 N_{2} + 2 B r^{-} + 6 H_{2} O$ .

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Solution

$3 N_{2} H_{4} + 2 B r O_{3}^{-} \to 3 N_{2} + 2 B r^{-} + 6 H_{2} O$ .
Oxidised- $N_{2} H_{4}$ The oxidation number of N increases from -2 to 0. Thus, N itself is oxidised and acts as reducing agent.
Reduced- $B r O_{3}^{-}$ . The oxidation number of Br decreases from +5 to -1. Thus, Br itself is reduced and acts as oxidising agent.

Note:
Any species that is oxidised acts as reducing agent.
Any species that is reduced acts as oxidising agent.

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