A sulphide of iron is formed by combining 1.296 gm of sulphur with 2.33 g of iron . what is compounds empirical formula
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Answer:
FeS
2
Explanation:
A sulphide of iron contains 46.5% of iron by weight.
100 g of sample will contain 46.5 g of iron and 100−46.5=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 =
55.8g/mol
46.5g
=0.8333.
The number of moles of sulphur =
32.1g/mol
53.5g
=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 FeS
2
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