Iron is extracted from iron(III) oxide in a blast furnace. The balanced equation for the reaction is:
Fe2O3+3CO→2Fe+3CO2 \text{Fe}_2\text{O}_3 + 3\text{CO} \rightarrow 2\text{Fe} + 3\text{CO}_2 Fe2O3+3CO→2Fe+3CO2Calculate the atom economy for the production of iron in this reaction.
Give your answer to two significant figures.
(Relative formula masses: Fe2O3=160\text{Fe}_2\text{O}_3 = 160Fe2O3=160, CO=28\text{CO} = 28CO=28, Fe=56\text{Fe} = 56Fe=56, CO2=44\text{CO}_2 = 44CO2=44)
119 exam-style questions on Edexcel GCSE Chemistry 6.2 Quantitative analysis, covering 6.2.1 Concentration in mol dm⁻³ and titration calculations, 6.2.2 Percentage yield and why actual yield falls short, 6.2.3 Atom economy of a reaction, 6.2.4 Choosing a reaction pathway, and 6.2.5 Molar volume of gases and Avogadro's law. Each one has a worked solution and a mark scheme showing where the marks go.