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Oxidation states of Iron

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2Fe(NH4)2(SO4)2*6H2O + 6K2C2O4 + H2O2 + H2SO4 ----

2K3[Fe(C2O4)3]*3H2O + 3K2SO4 + 2(NH4)2SO4 + 8H2O

I need to find the oxidation state of Iron in both the reagent side and product side of the equation.

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Recall that for a neutral compound the sum of the positive oxidation state and negative oxidation state must equal to zero.

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Solution Summary

The expert examines oxidation states of iron. The product side of the equations are discussed.The solution is given step-by-step.

See Also This Related BrainMass Solution

Redox Reaction: Ferrous Ion and Permanganate Ion

The ferrous ion, Fe2+(aq), reacts with the permanganate ion, MnO4- (aq), in an acidic solution to produce the ferric ion, Fe3+(aq). A 6.893 g sample of ore was mechanically crushed and tehn treated with concentrated hydrochloric acid, which oxidized all of the iron in the ore to the ferrous ion, Fe2+(aq). Next the acid solution containing all of the ferrous ions was titrated with .100 M KMnO4 solution. The end point was reached when 13.899mL of the KMnO4 solution was used.

a. Write the oxidation half reaction
b. Write the reduction half reaction
c. Write the balanced final redox reaction
d. Identify the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced
e. Calculate the number of moles of iron in the sample or ore
f. Calculate the mass percent of the iron in the ore

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