Iron is extracted from its ore, hematite (Fe2O3\text{Fe}_2\text{O}_3Fe2O3), in a blast furnace. Carbon monoxide reduces the iron(III) oxide to molten iron according to the reaction:
Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g) \text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 2\text{Fe}(l) + 3\text{CO}_2(g) Fe2O3(s)+3CO(g)→2Fe(l)+3CO2(g)Calculate the maximum amount, in moles, of iron (Fe\text{Fe}Fe) that could be formed from 240 kg240\text{ kg}240 kg of iron(III) oxide, assuming all of the iron(III) oxide is converted. (Take the relative atomic mass of Fe=56\text{Fe} = 56Fe=56 and O=16\text{O} = 16O=16.)
In practice, under specific blast furnace operating conditions, only 85%85\%85% of the iron(III) oxide is converted into iron. Calculate the actual amount, in moles, of iron formed from this reactant mixture.
80 exam-style questions on Edexcel IGCSE Chemistry Chemical formulae, equations and calculations. Each one has a worked solution and a mark scheme showing where the marks go.