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This electrochemical oxidation is what establishes the potential difference."},{"text":"The oxygen is oxidised electrochemically, setting up a potential difference across the terminals.","correct":false,"explanation":"Oxygen is reduced as it accepts electrons in the overall reaction. The fuel is oxidised electrochemically, creating the potential difference across the terminals."},{"text":"The fuel is burned thermally, setting up a potential difference across the terminals.","correct":false,"explanation":"Combustion releases heat but does not describe the electrode process responsible for the voltage. The fuel is oxidised electrochemically, which sets up the potential difference."}]},{"id":"89842103-2906-4436-8261-0d1eb7044cbc","cardType":"basic","points":1,"front":"When does an electric current flow from a fuel cell?","back":"When the terminals are joined in a complete circuit.","mcqOptions":null},{"id":"22e85c41-f717-43d3-bbb8-dba9b7f67f45","cardType":"basic","points":2,"front":"Why does a fuel cell not need recharging?","back":"Its reactants are supplied continuously from outside the cell.","mcqOptions":null},{"id":"1c2bb912-0a19-49e9-950f-ed9405a5b062","cardType":"basic","points":1,"front":"What happens if either the fuel or oxygen supply to a fuel cell stops?","back":"The cell stops producing a potential difference.","mcqOptions":[{"text":"The cell stops producing a potential difference.","correct":true,"explanation":"Without either reactant, the electrochemical reaction cannot continue, so charge separation stops and the fuel cell no longer produces a potential difference."},{"text":"The cell stops producing a chemical reaction.","correct":false,"explanation":"The wording asks what electrical effect stops. The missing reactant prevents the cell from producing a potential difference, although the reaction is also unable to continue."},{"text":"The cell starts producing a larger potential difference.","correct":false,"explanation":"Removing a reactant cannot increase the cell’s voltage; it stops the reaction needed to maintain it. The potential difference therefore ceases."},{"text":"The cell continues producing a potential difference.","correct":false,"explanation":"A continuous supply of both reactants is necessary to maintain the electrochemical reaction. 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Hydrogen and oxygen combine overall to produce water."},{"text":"Oxygen.","correct":false,"explanation":"Oxygen is a reactant consumed by the cell, not its chemical product. The only chemical product of the overall hydrogen fuel-cell reaction is water."}]},{"id":"ff34d36d-e6af-4d9d-806f-03d1201a889c","cardType":"basic","points":1,"front":"Why does a hydrogen fuel cell produce no carbon dioxide while running?","back":"Hydrogen contains no carbon.","mcqOptions":[{"text":"Hydrogen contains no carbon.","correct":true,"explanation":"Carbon dioxide can only form when carbon is present and oxidised. Hydrogen contains no carbon, so its reaction with oxygen produces water rather than carbon dioxide."},{"text":"Hydrogen contains no oxygen.","correct":false,"explanation":"The absence of oxygen in hydrogen is not why carbon dioxide is absent; oxygen is supplied separately from air. Hydrogen produces no carbon dioxide because it contains no carbon."},{"text":"Hydrogen contains no electrons.","correct":false,"explanation":"Hydrogen atoms and molecules do contain electrons, and electron transfer is central to the cell. No carbon dioxide forms because hydrogen contains no carbon."},{"text":"Hydrogen contains no protons.","correct":false,"explanation":"Hydrogen atoms contain protons, so this statement is scientifically false. The relevant fact is that hydrogen contains no carbon to form carbon dioxide."}]},{"id":"2719c93b-7eaf-4110-b269-2031ec1b04b0","cardType":"basic","points":2,"front":"Why can a hydrogen fuel cell run longer than a rechargeable battery?","back":"Fuel and oxygen are supplied continuously, whereas a battery contains a fixed amount of chemicals.","mcqOptions":null},{"id":"7a9d5b69-22f9-446b-8405-7cdcbda02cc1","cardType":"basic","points":3,"front":"How is a fuel cell returned to use, compared with a rechargeable battery?","back":"

A fuel cell is refilled with hydrogen.
A battery is connected to an electricity supply.

","mcqOptions":null},{"id":"45dd283e-c3f5-4278-92e6-ac412c5d8a37","cardType":"basic","points":2,"front":"Why is a hydrogen fuel cell not automatically environmentally harmless?","back":"Making and transporting hydrogen can use energy and release pollutants.","mcqOptions":null},{"id":"59e25e8a-36f4-49b4-a3f5-936c02d22bc7","cardType":"basic","points":2,"front":"What happens to hydrogen at the hydrogen electrode?","back":"Hydrogen loses electrons and is oxidised.","mcqOptions":null},{"id":"36da26e0-12d6-4fe3-9f85-803b5b3b2eca","cardType":"basic","points":2,"front":"What happens to oxygen at the oxygen electrode?","back":"Oxygen gains electrons and is reduced.","mcqOptions":null},{"id":"c15cccc6-cffe-470b-b1b1-70bcc7ee83de","cardType":"basic","points":1,"front":"On which side of an oxidation half equation are the electrons written?","back":"The products side.","mcqOptions":null},{"id":"00ebd906-29f1-44b2-9e97-8658dd3aee3c","cardType":"cloze","points":null,"front":"In a hydrogen fuel cell, hydrogen is [ ] and oxygen is reduced.","back":"In a hydrogen fuel cell, hydrogen is oxidised and oxygen is reduced.","mcqOptions":null},{"id":"99f9507d-27cb-4741-89c6-6f2621db023e","cardType":"cloze","points":null,"front":"The balanced hydrogen half equation is $\\text{H}_2\\text{(g)} \\rightarrow 2\\text{H}^+\\text{(aq)} + \\text{\\text{[...]}}$.","back":"The balanced hydrogen half equation is $\\text{H}_2\\text{(g)} \\rightarrow 2\\text{H}^+\\text{(aq)} + \\text{\\boxed{2e^-}}$.","mcqOptions":null},{"id":"45190d07-93af-4fc7-a7e1-d11d74b906ea","cardType":"cloze","points":null,"front":"The balanced oxygen half equation is $\\text{O}_2\\text{(g)} + 4\\text{H}^+\\text{(aq)} + \\text{\\text{[...]} \\rightarrow 2\\text{H}_2\\text{O(l)}$.","back":"The balanced oxygen half equation is $\\text{O}_2\\text{(g)} + 4\\text{H}^+\\text{(aq)} + \\text{\\boxed{4e^-} \\rightarrow 2\\text{H}_2\\text{O(l)}$.","mcqOptions":null},{"id":"f90c05ef-9901-4c88-bc1b-d1dcc975db88","cardType":"cloze","points":null,"front":"To combine the half equations, the hydrogen half equation is multiplied by [ ] so that four electrons are transferred.","back":"To combine the half equations, the hydrogen half equation is multiplied by two so that four electrons are transferred.","mcqOptions":null},{"id":"884f993a-7623-4865-b294-11f927f8d639","cardType":"cloze","points":null,"front":"After combining the half equations, the electrons and hydrogen ions are [ ] from both sides.","back":"After combining the half equations, the electrons and hydrogen ions are cancelled from both sides.","mcqOptions":null}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"5.2.2a Fuel cells","title":"5.2.2 Fuel cells Flashcards","topbar":{"backHref":"/gcse/chemistry/aqa/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"ccf24a4c-1709-5189-91eb-9f3f7352084e","walled":"$L38"}],"$L39","$L3a"]

5.2.2a Fuel cells Flashcards

5.2.2a Fuel cells Flashcards