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Energy changes are not just a topic in the chemistry lab — they are part of our daily lives. This lesson explores how exothermic and endothermic reactions are used in everyday products and situations, linking the theoretical concepts from AQA GCSE Chemistry to real-world applications. Understanding these applications will help you answer context-based questions in the exam.
Exothermic reactions release energy to the surroundings. Many products and processes rely on this energy release.
Disposable hand warmers contain iron powder, salt, water, activated charcoal, and vermiculite. When exposed to air (by opening the packaging), the iron undergoes a slow oxidation reaction:
iron + oxygen --> iron oxide
This reaction is exothermic and releases heat steadily over several hours.
| Feature | Detail |
|---|---|
| Reaction type | Oxidation (exothermic) |
| Reactants | Iron powder and oxygen from the air |
| Product | Iron oxide (rust) |
| Temperature reached | Approximately 40-50 degrees C |
| Duration | Up to 10 hours |
| Reusable? | No — the iron is fully oxidised |
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