$H_{2} S$ acts only as reducing agent while $S O_{2}$ can act both as reducing agent and oxidising agent. Explain.

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Solution

In $H_{2} S$ , $S$ is in its lowest oxidation state that is $- 2$ . Hence, it can only act as a reducing agent only.

In ${S O}_{2}$ , $S$ is in oxidation state that is $+ 4$ and its highest oxidation state is $+ 6$ . Hence, can act both as reducing agent and oxidising agent.

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$H_{2} S$ acts only as a reducing agent while $S O_{2}$ can act both as a reducing and oxidizing agent because

H N O_{3}

H N O_{2}

4 H C l + M n O_{2} \to M n C l_{2} + 2 H_{2} O + C l_{2}

{S O}_{2}

Identify the correct statement about $H_{2} O_{2}$

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