Question

The oxide, which cannot act as a reducing agent is:

• A. $C{O}_2$
• B. $Cl{O}_2$
• C. $N{O}_2$
• D. $S{O}_2$

Answer 1

The correct option is A $C{O}_2$

(a) Oxidation state of $C$ in $C{O}_2$ is $+4$. Since, carbon is in its maximum oxidation state of $+4$, therefore, carbon dioxide $\left(C{O}_2\right)$ cannot act as a reducing agent.
(b) Oxidation state of $Cl$ in $Cl{O}_2$ is $+4$. Since, chlorine is not in its maximum oxidation state, therefore, $\left(Cl{O}_2\right)$ can act as a reducing agent.
(c) Oxidation state of $N$ in $N{O}_2$ is $+4$. Since, nitrogen is not in its maximum oxidation state, therefore, $\left(N{O}_2\right)$ can act as a reducing agent.
(d) Oxidation state of $S$ in $S{O}_2$ is $+4$. Since, chlorine is not in its maximum oxidation state, therefore, $\left(S{O}_2\right)$ can act as a reducing agent.