In the industrial extraction of iron from its ore, carbon monoxide gas reacts with iron(III) oxide according to the following equation:
Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g) \text{Fe}_2\text{O}_3(\text{s}) + 3\text{CO}(\text{g}) \rightarrow 2\text{Fe}(\text{l}) + 3\text{CO}_2(\text{g}) Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g)Which statement correctly identifies the reducing agent in this reaction and explains its role in terms of electron transfer and oxidation states?
Fe2O3\text{Fe}_2\text{O}_3Fe2O3 is the reducing agent because iron gains electrons, and its oxidation state decreases from +3+3+3 to 000.
CO\text{CO}CO is the reducing agent because carbon gains electrons, and its oxidation state increases from +2+2+2 to +4+4+4.
CO\text{CO}CO is the reducing agent because carbon loses electrons, and its oxidation state increases from +2+2+2 to +4+4+4.
Fe2O3\text{Fe}_2\text{O}_3Fe2O3 is the reducing agent because it is reduced, and in doing so, it oxidises CO\text{CO}CO.
Practise OCR GCSE Chemistry Types of chemical reactions with exam-style questions for Foundation and Higher tier. 58 questions, matched to the OCR GCSE Chemistry (J248) specification and written in Paper 1 and Paper 2 (Foundation Tier) or Paper 3 and Paper 4 (Higher Tier) style. Every question includes a full worked solution and mark scheme, so you can see where marks are awarded rather than just whether you got the answer right.