A camping stove burns propane gas.
C3H8(g)+5O2(g)→3CO2(g)+4H2O(l)\mathrm{C_{3}H_{8}(g)} + \mathrm{5O_{2}(g)} \rightarrow \mathrm{3CO_{2}(g)} + \mathrm{4H_{2}O(l)}C3H8(g)+5O2(g)→3CO2(g)+4H2O(l)
One mole of any gas occupies 24 dm3\mathrm{dm^{3}}dm3 at room temperature and pressure (rtp). Relative formula masses: C3H8=44,CO2=44\mathrm{C_{3}H_{8}} = 44, \mathrm{CO_{2}} = 44C3H8=44,CO2=44
State what is meant by the molar volume of a gas.
Calculate the volume of 11.0 g of propane at rtp.
Calculate the volume of oxygen needed to burn this volume of propane completely. All volumes are measured at rtp.
Air contains 20 % oxygen by volume. Calculate the volume of air needed.
Calculate the mass of carbon dioxide formed when 11.0 g of propane burns completely.
Explain why the water produced is not included when gas volumes are calculated at rtp.
51 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.