Balance the following equations :
(a) MnO4- + Fe2+ + H+ →
(b) Cr2O7 2-+ Sn2+ + H+ →
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How much coulumb is required to convert MnO4^- into Mn^+2
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How much coulumb is required to convert MnO4^- into Mn^+2
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Number of moles of MnO4- required to oxidise one mole of ferrous oxalate completely in acidic medium will be:-
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...
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A compound Fe0.93O1.00, present find out the % of Fe2+ and Fe3+.
We have Fe3+=x and Fe2+=.93-x then using charge balance.. 3*x+2*(0.93-x)=2*1 ( 1 for oxygen) x=.14 % of Fe3+=(.14/.93)*100=15% % of Fe2+=(.79/.93)*100=85%
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Write the balanced redox reaction: a) MnO4 – (aq) + Fe2+ (aq) → Mn2+ (aq) + Fe3+ (aq)
(a) MnO4 – (aq) + 5Fe2+ (aq) + 8H+ (aq) → Mn2+ (aq) + 5Fe3+ (aq) + 4H2O(l) (b) Cr2O72– + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O.
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Identify the oxidizing and reducing agents in the following equations: a) MnO4 – (aq) + 5Fe2+ (aq) + 8H+ (aq) →
Oxidizing agent = MnO4 – and Reducing agent = Fe2+ Oxidizing agent = Cr2O7 2– and Reducing agent = Fe2+ .
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How much electricity is required in Coulomb for the oxidation of 1 mole of FeO to Fe2 O3 ?
Fe2+ => Fe3+ + 1e So, 1F = 1 x 96500 C = 96500 C
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Why Mn2+ compounds are more stable than Fe2+ compounds towards oxidation to their + 3 state ?
Mn+2 has half-filled electronic configuration.
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Why are Mn2+compounds more stable than Fe2+ towards oxidation to their +3 state?
Electronic configuration of Mn2+ is [Ar]18 3d5. Electronic configuration of Fe2+ is [Ar]18 3d6. It is known that half-filled and fully-filled orbitals are more stable. Therefore, Mn in (+2) state has a...
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Translate the following statements into chemical equations and then balance the equations:
(i) P4 + 5O2 -------> 2P2O5 (ii) 2Al + Fe2O3 -----> Al2O3+ 2Fe (iii) CS2 + 3O2 ------> CO2 + 2SO2 (iv) BaCl2 + ZnSO4 --------> ZnCl2 + BaSO4
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