Chemistry - Redox Reactions Question with Solution | TestHub
ChemistryRedox ReactionsDetermination of Oxidation StateMedium2 minQB
ChemistryMediummatching list
Match one mole of each oxidizing agent in Column I with the moles of reducing agent in Column II needed for complete reaction.
Column I | Column II |
|---|---|
A) KMnO₄ (H⁺) | P) 3.0 mole of FeSO₄ |
B) KMnO₄ (OH⁻) | Q) 0.5 mole of I₂ (oxidized to HIO₃) |
C) MnO₂ (H⁺) | R) 1.0 mole of K₂C₂O₄ |
D) K₂CrO₄ (H⁺) | S) 1.5 mole of K₂SO₃ |
Options:
Answer:
B
Solution:
Electrons supplied per mole of reductant: FeSO₄ (Fe²⁺ Fe³⁺) = 1; I₂ 2HIO₃ = 10; K₂C₂O₄ 2CO₂ = 2; K₂SO₃ K₂SO₄ = 2. (A) Mn(+7) Mn(+2) needs 5 e⁻: 0.5 mol I₂ supplies 5 (Q). (B) In OH⁻, Mn(+7) MnO₂ (+4) needs 3 e⁻: 3.0 mol FeSO₄ (P) or 1.5 mol K₂SO₃ (S) each supply 3. (C) MnO₂ (+4) Mn²⁺ needs 2 e⁻: 1.0 mol K₂C₂O₄ (R). (D) In H⁺, CrO₄²⁻ Cr(+6) Cr³⁺ needs 3 e⁻: 3.0 mol FeSO₄ (P) or 1.5 mol K₂SO₃ (S).
Stream:JEESubject:ChemistryTopic:Redox ReactionsSubtopic:Determination of Oxidation State
⏱ 2mℹ️ Source: QB
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