A reactor is supplied with methane and oxygen in the proportions needed for the reaction shown.
CH4(g)+2O2(g)→CO2(g)+2H2O(l) \mathrm{CH_{4}(g) + 2O_{2}(g) \rightarrow CO_{2}(g) + 2H_{2}O(l)} CH4(g)+2O2(g)→CO2(g)+2H2O(l)During one run, the reactor produces 60 cm3\mathrm{cm^{3}}cm3 of carbon dioxide. The gas volumes are compared at the same temperature and pressure.
What volumes of methane and oxygen react to make this carbon dioxide?
methane 60 cm3\mathrm{cm^{3}}cm3 and oxygen 60 cm3\mathrm{cm^{3}}cm3
methane 60 cm3\mathrm{cm^{3}}cm3 and oxygen 120 cm3\mathrm{cm^{3}}cm3
methane 120 cm3\mathrm{cm^{3}}cm3 and oxygen 60 cm3\mathrm{cm^{3}}cm3
methane 30 cm3\mathrm{cm^{3}}cm3 and oxygen 60 cm3\mathrm{cm^{3}}cm3
152 exam-style questions on OCR GCSE Chemistry 5.1 Monitoring chemical reactions, covering 5.1.1 The technique of titration, 5.1.2 Theoretical mass, percentage yield and atom economy, 5.1.3 Concentration of a solution in mol/dm3, 5.1.4 Concentration calculations and titration results, 5.1.5 Molar gas volume and volumes of gases in reactions, and 5.1.6 Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.