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Question

The weight of KMnO4 required to completely oxidise 0.25 moles of FeSO4 in acidic medium is:


[Molecular weight of KMnO4=158]

A
5.8
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B
1.5
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C
7.9
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D
0.79
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Solution

The correct option is C 7.9
The balanced chemical equation is as follows:
2KMnO4+3H2SO4+10FeSO4K2SO4+2MnSO4+5Fe2(SO4)3+3H2O.

2 moles (2×158 g) of KMnO4 completely oxidizes 10 moles of FeSO4.

The weight of KMnO4 required to completely oxidize 0.25 moles of FeSO4 will be (2×158)10×0.25=7.9 g.

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