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How many moles of Fe2 plus ion can be oxidized by 1.4x10-2 moles MnO4- ion?
Wiki User
∙ 13y ago
The molar mass of Fe2O3 is 55.845 (molar mass of iron)*2+16(molar mass of oxygen)*3, which comes out to be 159.69 grams per mole. Multiply that by the number of moles, and the answer is 223.57 grams.
Wiki User
∙ 13y ago
Wiki User
∙ 13y agoThe oxidation 1/2 reaction for iron is:
Fe2+ --> Fe3+ + e-
The reduction 1/2 reaction for permanganate is:
8H+ + MnO4- + 5e- --> Mn2+ + 4H2O
From this we can see that 5 moles of iron can be oxidized for every mole of permanganate that can be reduced.
In other words... 5 times as much iron can be oxidized as there is permanganate present.
Therefore the amount of Fe2+ that can be oxidized is:
1.4x10-2 mol x 5 = 7.0x10-2 mol.
Answer: 7.0x10-2 mol of Fe2+
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