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Question

A sulphide of iron contains 46.5% of iron by weight. The empirical formula of the sulphide is:

A
FeS
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B
Fe2S
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C
FeS2
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D
Fe2S3
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Solution

The correct option is D FeS2
A sulphide of iron contains 46.5% of iron by weight.
100 g of sample will contain 46.5 g of iron and 10046.5=53.5 g of sulphur.
The atomic masses of iron and sulphur are 55.8 g/mol and 32.1 g/mol.
The number of moles of iron =46.5g55.8g/mol=0.8333.
The number of moles of sulphur =53.5g32.1g/mol=1.667
The ratio of the number of moles of iron to the number of moles of sulphur =0.8333:1.667=1:2
Hence, the empirical formula of the sulphide is FeS2.

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