A fuel cell car has a tank that holds 5.0 kg of hydrogen. On a full tank the car can travel 600 km.
2H2(g)+O2(g)→2H2O(l)2\mathrm{H_{2}(g)} + \mathrm{O_{2}(g)} \rightarrow 2\mathrm{H_{2}O(l)}2H2(g)+O2(g)→2H2O(l)
Relative atomic masses: H = 1, C = 12, O = 16. The volume of one mole of any gas at room temperature and pressure is 24 dm3\mathrm{dm^{3}}dm3.
Calculate the volume, in dm3\mathrm{dm^{3}}dm3, that 5.0 kg of hydrogen would occupy at room temperature and pressure.
Use your answer to (a) to explain why the hydrogen in the car is stored at a very high pressure.
Calculate the mass of water, in g, produced for each kilometre the car travels.
The hydrogen for the car is made from methane.
CH4(g)+2H2O(g)→CO2(g)+4H2(g)\mathrm{CH_{4}(g)} + 2\mathrm{H_{2}O(g)} \rightarrow \mathrm{CO_{2}(g)} + 4\mathrm{H_{2}(g)}CH4(g)+2H2O(g)→CO2(g)+4H2(g)
Calculate the mass, in kg, of carbon dioxide released when 5.0 kg of hydrogen is made by this reaction.
A petrol car releases 120 g of carbon dioxide for each kilometre it travels. Evaluate the claim that the fuel cell car is a zero-emission vehicle. Use your answer to (d) and a calculation in your answer.
38 exam-style questions on Edexcel GCSE Chemistry 6.4 Chemical cells and fuel cells, covering 6.4.1 Chemical cells and fuel cells. Each one has a worked solution and a mark scheme showing where the marks go.