A camping stove burns butane, C4H10\mathrm{C_{4}H_{10}}C4H10. The butane undergoes complete combustion when there is plenty of air.
Relative formula mass: C4H10=58\mathrm{C_{4}H_{10}} = 58C4H10=58. One mole of any gas occupies 24 dm3\mathrm{dm^{3}}dm3 at room temperature and pressure.
Write the balanced equation for the complete combustion of butane.
The stove burns 29.0 g of butane. Calculate the volume of carbon dioxide produced at room temperature and pressure.
Air contains 20% oxygen by volume. Calculate the minimum volume of air needed for the complete combustion of 29.0 g of butane.
The instructions warn that the stove must never be used inside a closed tent.
Write a balanced equation for the incomplete combustion of butane to form carbon monoxide and water only.
Explain why carbon monoxide is dangerous to people in the tent.
36 exam-style questions on Edexcel GCSE Chemistry 10.2 Hydrocarbons, covering 10.2.1 Formulae and structures of the alkanes, 10.2.2 Alkenes and the C=C functional group, 10.2.3 Addition reactions of alkenes and testing for unsaturation, and 10.2.4 Combustion of alkanes and alkenes. Each one has a worked solution and a mark scheme showing where the marks go.