1.1. Iron is extracted from haematite by reduction.

Name the substance used to carry out the reduction.

Give a reason why it is used.

Substance

Reason

1.2. Haematite is impure iron(III) oxide, Fe₂O₃.

Calculate the relative formula mass of iron(III) oxide.

1.3. Which substance is reduced in the extraction of iron from iron(III) oxide?

Tick (✓) one box

1.4. Another ore of iron is limonite, FeO(OH)•H₂O.

Give the total number of atoms in the formula.

Number of atoms

1.5. Calculate the percentage of iron in limonite.

Give your answer to three significant figures.

(M_r of FeO(OH)•H₂O = 107)

1.6. Iron reacts with sulfuric acid to form iron(III) sulfate and hydrogen.

Balance the reaction equation:

2Fe + H₂SO₄ → Fe₂(SO₄)₃ + H₂

1.7. Copper can be displaced from copper(II) sulfate solution by iron in this reaction:

Fe + CuSO₄ → FeSO₄ + Cu

How much copper can be made from 2.8 g of iron?

Relative atomic mass (A_r): Cu = 63.5, Fe = 56