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(A) The oxidation state of $S$ in $SO_2$ is $+4$. The range of oxidation states for $S$ is from $-2$ to $+6$. Since the oxidation state of $S$ in $SO_

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$SO_2$

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(A) The oxidation state of $S$ in $SO_2$ is $+4$. The range of oxidation states for $S$ is from $-2$ to $+6$. Since the oxidation state of $S$ in $SO_2$ $(+4)$ lies between its minimum $(-2)$ and maximum $(+6)$ oxidation states,it can either be oxidized to $+6$ or reduced to $-2$. Therefore,$SO_2$ can act as both an oxidizing and a reducing agent.

Which compound acts as an oxidising as well as reducing agent?

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