Justify that the following reactions are redox reactions:

$F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)$

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Solution

The oxidation number of iron( $F e$ ) decreases from $+ 3$ to $0$ . The oxidation number of $C$ increases from $+ 2$ to $+ 4$ .

Hence, $F e_{2} O_{3}$ is reduced and $C O$ is oxidized.

Hence, it is a redox reaction.

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Similar questions

Justify that the following reactions are redox reactions:

(a) CuO(s) + H₂(g) → Cu(s) + H₂O(g)

(b) Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)

(d) 2K(s) + F₂(g) → 2K+F– (s)

(e) 4 NH₃(g) + 5 O₂(g) → 4NO(g) + 6H₂O(g)

Q. The following two reactions are known

F e_{2} O_{3 (s)} + 3 C O_{(g)} \to 2 F e (s) + 3 C O_{2 (g)}

;

Δ H = - 26.8 k J

F e O_{(s)} + C O_{(g)} \to F e_{(s)} + C O_{2 (g)} Δ H = - 16.5 k J

The value of

Δ H

for the following reaction is:

F e_{2} O_{3 (s)} + C O_{(g)} \to 2 F e O_{(s)} + C O_{2 (g)}

Q. Find the value of

Δ H^{\circ}

for the reaction,

F e_{2} O_{3} (s) + 3 C O_{2} (g) \to 2 F e (s) + 3 C O_{2} (g)

Q. For the reaction,

F e_{2} O_{3} (s) + 3 C O (g) \to 3 C O_{2} (g) + 2 F e (l)

which of the following is correct?

2 H_{2} S (g) + 3 O_{2} (g) \to 2 S O_{2} (g) + 2 H_{2} O (g) +

heat

F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)

According to the above reaction , 3 moles of $F e_{2} O_{3}$ are allowed react with 56 grams of CO so, find the approximately moles of iron produced ?

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Justify that the following reactions are redox reactions:Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

The oxidation number of iron(Fe) decreases from +3 to 0. The oxidation number of C increases from +2 to +4. Hence, Fe2O3 is reduced and CO is oxidized. Hence, it is a redox reaction.

Justify that the following reactions are redox reactions:

$F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)$

The oxidation number of iron( $F e$ ) decreases from $+ 3$ to $0$ . The oxidation number of $C$ increases from $+ 2$ to $+ 4$ .

Hence, $F e_{2} O_{3}$ is reduced and $C O$ is oxidized.

Hence, it is a redox reaction.