The oxide which cannot act as a reducing agent is__________.

S O_{2}

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N O_{2}

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C O_{2}

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C l O_{2}

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Solution

The correct option is C $C O_{2}$
A substance can acts as the reducing agent when it can increase its oxidation state by losing electrons.
In $S O_{2}$ , sulphur is present in +4 oxidation state it can increase its oxidation state up to +6 so it can act as a reducing agent.
In $N O_{2}$ , nitrogen is present in +4 oxidation state it can increase its oxidation state up to +5 so it can act as a reducing agent.
In $C O_{2}$ , carbon is present in +4 oxidation state which is its maximum oxidation state so it cannot acts as a reducing agent.
In $C l O_{2}$ , chlorine is present in +4 oxidation state it can increase its oxidation state up to +7 so it can act as a reducing agent.

Hence, the correct option is $C$

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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

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