Suppose that an endpoint is reacted when 30 moles of KMnO4 was added. How many moles of Fe^2+ was there originally.
I thought the answer was 150 moles.
Identify the Oxidation and reduction half reaction in 2 KMNO4 + 10 FeSO4 + 8 H2SO4 -> K2SO4 + 2 MNSO4 + 5 Fe2(SO4)3 + 8 H2O
Write net ionic equation
2 answers
Oxidation is the loss of electrons. So Fe goes from +2 on the left to +3 on the right and Mn goes from +7 on the left to +2 on the right. Which loses electrons. You try writing the equations.
If you have 30 mols KMnO4 you must have reacted it with 30 x 10/2 = ? and that sure looks like 150 to me.
If you have 30 mols KMnO4 you must have reacted it with 30 x 10/2 = ? and that sure looks like 150 to me.
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