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Fuel cells are electrochemical devices that convert the chemical energy of a fuel directly into electrical energy. This is a Higher Tier topic in the AQA GCSE Chemistry specification. You need to understand how hydrogen fuel cells work, their advantages and disadvantages compared to conventional cells and batteries, and their applications in modern technology.
A fuel cell is an electrochemical cell in which a fuel (usually hydrogen) and an oxidant (usually oxygen from the air) react to produce electricity, with water as the only product.
Unlike a conventional cell or battery, a fuel cell does not run down or need recharging — it continues to produce electricity as long as fuel and oxygen are supplied.
The overall reaction in a hydrogen fuel cell is:
hydrogen + oxygen --> water
2H2 + O2 --> 2H2O
| Feature | Detail |
|---|---|
| Fuel | Hydrogen gas (H2) |
| Oxidant | Oxygen gas (O2) from the air |
| Product | Water (H2O) — the only chemical product |
| Energy output | Electrical energy (and some heat) |
| Waste | Water — no carbon dioxide, no pollutants |
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