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Question

How many gram of iron pyrite (FeS2) should be burnt completely to produce SO2 gas needed to decolorize completely 100ml, 0.12M, KMnO4 solution in acidic medium. [Fe= 56]

A
1.2gm
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B
1.8gm
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C
0.9gm
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D
00.36gm
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Solution

The correct option is D 1.8gm
2FeS2+112O2Fe2O3+4SO2
MnO4+SO2Mn+2+SO3
Balance above reaction
2MnO4+5SO2+6H+2Mn+2+5SO3+3H2O
Number of mole of MnO4=0.12×100ml
=12mMol
2molMnO4 required 5molSO2
12mmolMnO4 required 52×12mMol
=30mMol
Now,
4molSO2 required 2molFeS2
30mMolSO2 required 24×30mol
15mmol
Amount of FeS2=15×103×(56+64)
=120×15×103
=1.8g

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