Justify that the reactions is redox reactions: $\left.\mathrm{Fe}_{2} \mathrm{O}_{3} \mathrm{~s}\right)+3 \mathrm{CO}_{(g)} \rightarrow 2 \mathrm{Fe}_{(s)}+3 \mathrm{CO}_{2}(\mathrm{~g})$

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Justify that the reactions is redox reactions: $\left.\mathrm{Fe}_{2} \mathrm{O}_{3} \mathrm{~s}\right)+3 \mathrm{CO}_{(g)} \rightarrow 2 \mathrm{Fe}_{(s)}+3 \mathrm{CO}_{2}(\mathrm{~g})$

Solution:

$\mathrm{Fe}_{2} \mathrm{O}_{3(s)}+3 \mathrm{CO}_{(g)} \rightarrow 2 \mathrm{Fe}_{(s)}+3 \mathrm{CO}_{2}(g)$
In the above response,
Oxidation no. of Fe and $\mathrm{O}$ in $\mathrm{Fe}_{2} \mathrm{O}_{3}$ is $+3$ and $-2$ separately.
Oxidation no. of $\mathrm{C}$ and 0 in $\mathrm{CO}$ is $+2$ and $-2$ individually.
Oxidation no. of Fe is 0 .
Oxidation no. of $\mathrm{C}$ and $\mathrm{O}$ in $C O_{2}$ is $+4$ and $-2$ individually.
The oxidation no. of Fe diminished from $+3$ in $\mathrm{Fe}_{2} \mathrm{O}_{3}$ to 0 in $\mathrm{Fe}$ . That is $\mathrm{Fe}_{2} \mathrm{O}_{3}$ is decreased to $\mathrm{Fe}$ .
The oxidation no. of $\mathrm{C}$ expanded from 0 to $+2$ in $\mathrm{CO}$ to $+4$ in $\mathrm{CO}_{2}$ . That is $\mathrm{CO}$ is oxidized to $\mathrm{CO}_{2}$ .
In this way, the response is redox response.