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Question

# One line of an acidified solution of KMnO4 containing 15 g of KMnO4 is decolourised by passing sufficient amount of SO2. If SO2 is produced by roasting of iron pyrites (FeS2) and X g amount of pyrites is required to produce the necessary amount of SO2, then what is the value of X?

A
15
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B
20
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C
10
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D
None of these
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Solution

## The correct option is A 15The reaction for the roasting of FeS2 is as follows:4FeS24×120+11O2→2Fe2O3+8SO28×64Equivalents of KMnO4=15.031.6×1 L=0.5 eq. of KMnO4 =0.5eq of SO2 =0.5×642g of SO2 =16 g of SO28×64 g of SO2 is produced from 2×120 g of FeS2. (from the equation above)∴16 g of SO2 is produced from 4×1208×64×64=15 g.

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