🎯 Common Question Types:
- Write/complete the overall equation for the fuel cell (1–2 marks)
- Write the half-equation at anode or cathode (1 mark each)
- Evaluate fuel cells vs batteries — give advantages AND limitations (3–4 marks)
- Explain voltage in terms of reactivity difference (2 marks)
📝 Key Command Words:
- State — just name it, no explanation needed
- Write — give the equation with correct formulae and balancing
- Explain — give the chemical reason (e.g. "because electrons flow from the more reactive metal...")
- Evaluate — give advantages AND disadvantages with a reasoned judgement
- Compare — say something about BOTH items being compared
⚠️ Common Mistakes to Avoid:
- Confusing anode and cathode polarity (anode = negative = oxidation in a fuel cell)
- Saying fuel cells "produce no environmental impact" — they only produce water at point of use; hydrogen production may use fossil fuels
- Forgetting to balance the overall equation: 2H₂ + O₂ → 2H₂O (not H₂ + O₂ → H₂O)
- Stating that using the same metal in a cell "reduces voltage" — it gives zero voltage, not just less
This exam tips covers Exam Tips within Fuel Cells for GCSE Chemistry. Revise Fuel Cells in Energy Changes for GCSE Chemistry with 5 exam-style questions and 6 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 12 of 13 in this topic. Treat this as a marking guide for what examiners are looking for, not just a fact list.
Practice questions for Fuel Cells
A simple electrochemical cell is made by placing two different metal electrodes into an electrolyte. Which statement correctly describes what affects the voltage produced?
Compare a non-rechargeable alkaline battery with a rechargeable lithium-ion battery. Give one advantage and one disadvantage of the rechargeable battery.
Quick recall flashcards
Write the overall equation for the hydrogen–oxygen fuel cell.
2H₂ + O₂ → 2H₂O
Only product: water.
No carbon dioxide or air pollutants produced at point of use.
What is a fuel cell?
An electrochemical cell that generates electricity continuously from an external fuel supply (hydrogen) and an oxidant (oxygen).
Unlike a battery, it does not run down — it operates as long as fuel is supplied.
Only product: water.