In industrial metallurgy, iron is extracted from its ore, hematite (Fe2O3\text{Fe}_2\text{O}_3Fe2O3), in a blast furnace. The main reduction reaction is:
Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g) \text{Fe}_2\text{O}_3\text{(s)} + 3\text{CO(g)} \rightarrow 2\text{Fe(l)} + 3\text{CO}_2\text{(g)} Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g)What is the atom economy for the production of iron in this process?
Relative formula masses (MrM_rMr): Fe2O3=159.6\text{Fe}_2\text{O}_3 = 159.6Fe2O3=159.6, CO=28.0\text{CO} = 28.0CO=28.0, Fe=55.8\text{Fe} = 55.8Fe=55.8, CO2=44.0\text{CO}_2 = 44.0CO2=44.0
22.9%22.9\%22.9%
29.7%29.7\%29.7%
45.8%45.8\%45.8%
59.5%59.5\%59.5%
81 exam-style questions on OCR GCSE Chemistry Improving processes and products. Each one has a worked solution and a mark scheme showing where the marks go.