Indicate which of the substance/ion in the following reaction is an oxidising agent and which is a reducing agent?
$S O_{2} + C l_{2} + 2 H_{2} O \to 2 H C l + H_{2} S O_{4}$ .

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Solution

$S O_{2} + C l_{2} + 2 H_{2} O \to 2 H C l + H_{2} S O_{4}$ .
Oxidising agent- $C l_{2}$ The oxidation number of Cl decreases from 0 to -1. Thus, Cl itself is reduced.
Reducing agent- $S O_{2}$ . The oxidation number of S increases from +4 to +6. Thus, S itself is oxidised.

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

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