CCEA GCSE Chemistry
CCEA GCSE Chemistry 2.2 Redox, Rusting and Iron Exam Questions
Free CCEA GCSE Chemistry revision for 2.2 Redox, Rusting and Iron: what you need to know, common mistakes and exam-style questions with answers. Covers oxidation and reduction in terms of oxygen, hydrogen and electrons, rusting and its prevention, and the blast furnace.
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About CCEA GCSE Chemistry 2.2 Redox, Rusting and Iron
Redox, Rusting and Iron is a Unit 2 topic in CCEA GCSE Chemistry. It defines oxidation and reduction in three ways (oxygen, hydrogen and electron transfer) and asks you to identify what is oxidised and reduced, and the oxidising and reducing agents, in a reaction. You then apply these ideas to rusting, the conditions needed for it, and methods of rust prevention including sacrificial protection. The topic finishes with the extraction of iron from haematite in the blast furnace, including the role of each raw material. It builds on the reactivity series and links to electrolysis. Examiners often ask for blast furnace equations, rust experiments and redox definitions.
What you need to know
- Redox definitions Oxidation is gain of oxygen, loss of hydrogen or loss of electrons. Reduction is loss of oxygen, gain of hydrogen or gain of electrons (OIL RIG). A reducing agent is oxidised and an oxidising agent is reduced.
- Rusting Iron rusts when it is in contact with both water and oxygen, forming hydrated iron(III) oxide. Salt water speeds up rusting. Experiments compare nails in air and water, boiled water with oil on top (no oxygen) and dry air with calcium chloride (no water).
- Preventing rust Barrier methods (painting, oiling, greasing, plastic coating) keep out water and oxygen. Galvanising coats iron with zinc. Sacrificial protection attaches a more reactive metal such as magnesium or zinc, which is oxidised instead of the iron.
- Blast furnace raw materials Iron ore (haematite, Fe2O3), coke (carbon), limestone (CaCO3) and hot air are used. Molten iron and slag are tapped from the bottom.
- Blast furnace reactions C + O2 → CO2 provides heat. CO2 + C → 2CO makes the reducing agent. Fe2O3 + 3CO → 2Fe + 3CO2 reduces the ore. Limestone decomposes, CaCO3 → CaO + CO2, and CaO + SiO2 → CaSiO3 removes sandy impurities as slag.
Common mistakes in 2.2 Redox, Rusting and Iron
- Saying iron needs only water or only oxygen to rust. Both must be present.
- Explaining galvanising only as a barrier. Zinc also gives sacrificial protection, so it still protects if the coating is scratched.
- Identifying the reducing agent as the substance that is reduced. The reducing agent is itself oxidised.
- Writing carbon as the main reducing agent for iron oxide in the blast furnace. It is carbon monoxide.
- Saying limestone removes impurities directly. It decomposes to calcium oxide, which reacts with silicon dioxide to form slag.
Try three 2.2 Redox, Rusting and Iron exam-style questions
1. In the reaction Fe2O3 + 3CO → 2Fe + 3CO2, identify the substance oxidised and the substance reduced, explaining your answers. (4 marks)
Show the mark scheme answer
Carbon monoxide is oxidised; it gains oxygen; iron(III) oxide is reduced; it loses oxygen.
2. Explain why attaching blocks of magnesium to a steel ship's hull prevents rusting. (3 marks)
Show the mark scheme answer
Magnesium is more reactive than iron; it is oxidised or corrodes instead of the iron; sacrificial protection.
3. Calculate the mass of iron that can be obtained from 1000 kg of iron(III) oxide, Fe2O3. (Ar Fe = 56, O = 16) (3 marks)
Show the mark scheme answer
Mr Fe2O3 = 160; mass of iron in it = 112 / 160 of the total; 112 / 160 x 1000 = 700 kg.
2.2 Redox, Rusting and Iron FAQs
What does CCEA GCSE Chemistry 2.2 Redox, Rusting and Iron cover?
It covers oxidation and reduction in terms of oxygen, hydrogen and electrons, the conditions for rusting, methods of rust prevention and the extraction of iron in the blast furnace.
Which unit is 2.2 Redox, Rusting and Iron examined in?
It is examined in the Unit 2 written paper, Further Chemical Reactions, Rates and Equilibrium, Calculations and Organic Chemistry.
Which equations should I learn for the blast furnace?
Learn the five equations: burning coke, forming carbon monoxide, reducing iron(III) oxide, decomposing limestone and forming slag. Practise writing them balanced from memory.
