A. 7.5 moles B. 0.2 moles C. 0.6 moles D. 0.4 moles
Answered Feb 05, 2023
Here is Reaction with Balance
10FeC2O4 + 6KMnO4 + 24H2SO4 ----> 3K2SO4+ 6MnSO4 + 5Fe2(SO4)3 + 24H2O + 20CO2
So we see that
6 moles of KMnO4 is required to oxidize 10 moles of FeC2O4
Then, 1 mole of FeC2O4 would be oxidized by = ?
6/10=0.6
Please recheck your question
(a) √3/√2 is the correct option
(a) MnO4 – (aq) + 5Fe2+ (aq) + 8H+ (aq) → Mn2+ (aq) + 5Fe3+ (aq) + 4H2O(l) (b) Cr2O72– + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O.
Oxidizing agent = MnO4 – and Reducing agent = Fe2+ Oxidizing agent = Cr2O7 2– and Reducing agent = Fe2+ .
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Cl2 < MnO4 _ < Ce4+
Due to charge transfer complex formation.
(a) MnO4 - + Fe2+ + H+ → Mn+2 + Fe+3 (b) Cr2O7 2- + Sn2+ + H+→ Cr+3 + Sn+4
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