Justify that the following reaction is redox reaction: \[\ce{Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)}\]

\[\ce{Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)}\] Let us write the oxidation number of each element in the given reaction as: \[\ce{^{+3}Fe2^{-2}O3(s) + 3^{+2}C^{-2}O(g) → 2^{0}Fe(s) + 3^{+4}C^{-2}O2(g)}\] Here, the oxidation number of Fe decreases from +3 in Fe2O3 to 0 in Fe i.e., Fe2O3 is reduced to Fe. On the other hand, the oxidation number of C increases from +2 in CO to +4 in CO2 i.e., CO is oxidized to CO2. Hence, the given reaction is a redox reaction.

Justify that the following reaction is redox reaction: FeX2OX3(s)+3CO(g)⟶2Fe(s)+3COX2(g) - Chemistry

प्रश्न

Justify that the following reaction is redox reaction:

$Fe_{2} O_{3} (s) + 3 CO (g) ⟶ 2 Fe (s) + 3 CO_{2} (g)$

संख्यात्मक

उत्तर

$Fe_{2} O_{3} (s) + 3 CO (g) ⟶ 2 Fe (s) + 3 CO_{2} (g)$

Let us write the oxidation number of each element in the given reaction as:

$_{}^{}_{}^{+ 3} Fe_{2}^{- 2} O_{3} (s) + 3^{+ 2} C^{- 2} O (g) ⟶ 2^{0} Fe (s) + 3^{+ 4} C^{- 2} O_{2} (g)$

Here, the oxidation number of Fe decreases from +3 in Fe₂O₃ to 0 in Fe i.e., Fe₂O₃ is reduced to Fe. On the other hand, the oxidation number of C increases from +2 in CO to +4 in CO₂ i.e., CO is oxidized to CO₂. Hence, the given reaction is a redox reaction.

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Oxidation Number - Types of Redox Reactions

क्या इस प्रश्न या उत्तर में कोई त्रुटि है?

Q 8.3 - (b)Q 8.3 - (a)Q 8.3 - (c)

अध्याय 8: Redox Reactions - EXERCISES [पृष्ठ २८०]

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एनसीईआरटी Chemistry - Part 1 and 2 [English] Class 11

अध्याय 8 Redox Reactions
EXERCISES | Q 8.3 - (b) | पृष्ठ २८०

संबंधित प्रश्न

Justify that the following reaction is redox reaction:

$2 K (s) + F_{2} (g) ⟶ 2 K^{+} F^{-} (s)$

Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:

$2 AgBr (s) + C_{6} H_{6} O_{2} (aq) ⟶ 2 Ag (s) + 2 HBr (aq) + C_{6} H_{4} O_{2} (aq)$

Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:

$HCHO (l) + 2 [Ag (NH_{3})_{2}]^{+} (aq) + 3 OH^{-} (aq) ⟶ 2 Ag (s) + HCOO^{-} (aq) + 4 NH_{3} (aq) + 2 H_{2} O (l)$

Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:

$HCHO (l) + 2 Cu^{2 +} (aq) + 5 OH^{-} (aq) ⟶ Cu_{2} O (s) + HCOO^{-} (aq) + 3 H_{2} O (l)$

Consider the reactions:

$2 S_{2} O_{3}^{(2 -)} (aq) + l_{2} (S) ⟶ S_{4} O_{6}^{(2 -)} (aq) + 2 l^{-} (aq)$

$S_{2} O_{3}^{(2 -)} (aq) + 2 Br_{2} (l) + 5 H_{2} O (l) ⟶ 2 SO_{4}^{2 -} (aq) + 4 Br^{-} (aq) + 10 H^{+} (aq)$

Why does the same reductant, thiosulphate react differently with iodine and bromine?

Why does the following reaction occur?

$XeO_{6}^{4 -} (aq) + 2 F^{-} (aq) + 6 H^{+} (aq) ⟶ XeO_{3} (g) + F_{2} (g) + 3 H_{2} O (l)$

What conclusion about the compound Na₄XeO₆ (of which ${XeO}_{6}^{4 +}$ is a part) can be drawn from the reaction.

What sorts of informations can you draw from the following reaction ?

$(CN)_{2 (g)} + 2 OH^{-}_{(aq)} ⟶ CN^{-}_{(aq)} + CNO^{-}_{(aq)} + H_{2} O_{(l)}$

Refer to the periodic table given in your book and now answer the following question:

Select three metals that can show disproportionation reaction.

Which of the following is not an example of redox reaction?

Which of the following elements does not show disproportionation tendency?

Why does fluorine not show disporportionation reaction?

Write redox couples involved in the reactions given.

$Mg + Fe^{2 +} ⟶ Mg^{2 +} + Fe$

Write redox couples involved in the reactions given.

$Br_{2} + 2 Cl^{-} ⟶ Cl_{2} + 2 Br^{-}$

Which of the following examples does not represent disproportionation?

An acidified manganate solution undergoes disproportionation reaction. The spin-only magnetic moment value of the product having manganese in a higher oxidation state is ______ B.M. (Nearest integer)

For the decomposition reaction $NH_{2} COONH_{4} (s) \overset{- ⇀}{↽ -} 2 NH_{3} (g) + CO_{2} (g)$ the K_p = 2.9 × 10^-5 atm³. The total pressure of gases at equilibrium when 1 mol of $NH_{2} COONH_{4} (s)$ was taken initially could be ______.

Justify that the following reaction is redox reaction: FeX2OX3(s)+3CO(g)⟶2Fe(s)+3COX2(g) - Chemistry

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Justify that the following reaction is redox reaction: FeX2OX3(s)+3CO(g)⟶2Fe(s)+3COX2(g) - Chemistry

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