Empirical formula of a oxide of iron which has 69.9%iron and 30.1%dioxygen by mass
Answers
Answer:
100 g of the compound contains 69.9 g iron and 30.1 g oxygen.
The atomic masses of iron and oxygen are 55.85 amu and 16.00 amu.
The number of moles of Fe present in 100 g of compound are
55.85
69.9
=1.25
The number of moles of O present in 100 g of compound are
16.00
30.1
=1.88
The mole ratio of Fe to O is
1.88
1.25
=0.67:1 or 2:3
Hence, the empirical formula is Fe
2
O
3
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Answer:
Explanation:
100 g of the compound contains 69.9 g iron and 30.1 g oxygen.
The atomic masses of iron and oxygen are 55.85 amu and 16.00 amu.
The number of moles of Fe present in 100 g of compound are
55.85
69.9
=1.25
The number of moles of O present in 100 g of compound are
16.00
30.1
=1.88
The mole ratio of Fe to O is
1.88
1.25
=0.67:1 or 2:3
Hence, the empirical formula is Fe is 2
And oxygen is 3.