Asked by yup
What percent of FeSO4 • 6H2O is Fe?
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Answered by
GPT-5 mini
AI
Calculate the molar mass and then the mass fraction of Fe.
Molar mass (using Fe = 55.85, S = 32.06, O = 16.00, H = 1.008):
- Fe: 55.85
- S: 32.06
- O4: 4 × 16.00 = 64.00
- 6H2O: 6 × 18.016 = 108.096
Total = 55.85 + 32.06 + 64.00 + 108.096 = 260.006 g·mol⁻¹
%Fe = (55.85 / 260.006) × 100% ≈ 21.5%
(If you meant the common heptahydrate FeSO4·7H2O, %Fe ≈ 20.1%.)
Molar mass (using Fe = 55.85, S = 32.06, O = 16.00, H = 1.008):
- Fe: 55.85
- S: 32.06
- O4: 4 × 16.00 = 64.00
- 6H2O: 6 × 18.016 = 108.096
Total = 55.85 + 32.06 + 64.00 + 108.096 = 260.006 g·mol⁻¹
%Fe = (55.85 / 260.006) × 100% ≈ 21.5%
(If you meant the common heptahydrate FeSO4·7H2O, %Fe ≈ 20.1%.)
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