☰ Year plan · Chemistry

Iron and its oxides

Week 5 · Chapter 1 (E): pure iron and its +2 and +3 states, the reactions of iron (air, steam, chlorine, sulphur, acids, passivity) and the three oxides of iron with their preparation and properties (paper equations and calculations only) · 3 lessons
Answers are for parents and teachers.
1
Fe + H₂SO₄ → FeSO₄ + H₂. For 22.4 g of iron (Fe = 56, S = 32, O = 16) find the volume of hydrogen at STP (22.4 L/mol) and the mass of FeSO₄ (M = 152 g/mol).
2
Fe₂O₃ + 3H₂SO₄ → Fe₂(SO₄)₃ + 3H₂O. For 32 g of Fe₂O₃ (H = 1, S = 32, O = 16) find the mass of acid needed and of Fe₂(SO₄)₃ formed (M = 400 g/mol).
3
2Fe(OH)₃ → Fe₂O₃ + 3H₂O. What mass of Fe(OH)₃ (M = 107 g/mol) must be heated on paper to give 8.0 g of Fe₂O₃ (M = 160 g/mol)?
4
Fe₃O₄ + CO → 3FeO + CO₂. For 11.6 g of Fe₃O₄ (C = 12, O = 16) find the mass of FeO formed, of CO needed and of CO₂ formed.
5
A pupil says: “Fe₃O₄ is iron(II) oxide because it is black, like FeO.” Correct this in two sentences.