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Energy Changes & Reversible Reactions (AQA GCSE Chemistry: Combined Science)
Revision Note
Energy changes & reversible reactions
- Energy changes also accompany chemical changes and energy can be given out (exothermic) or taken in (endothermic)
- The majority of chemical reactions are exothermic with only a small number being endothermic
- For a reversible reaction, if it is exothermic in one direction then it must be endothermic in the opposite direction
- The amount of energy transferred in either direction is the same
- Reversible reactions can be seen in some hydrated salts
- These are salts that contain water of crystallisation which affects their shape and colour
- Water of crystallisation is the water that is included in the structure of some salts during the crystallisation process
- Water of crystallisation is indicated with a dot written in between the salt and the surrounding water molecules
- Anhydrous salts are those that have lost their water of crystallisation, usually by heating, in which the salt becomes dehydrated
Reversible reaction example
- A common example is copper(II) sulfate which crystallises forming the salt copper(II) sulfate pentahydrate, CuSO4.5H2O
- If hydrated copper(II) sulfate crystals are heated, the blue crystals turn into a white powder and a clear, colourless liquid (water) collects at the top of the test tube
- This forward reaction is endothermic
- When anhydrous copper(II) sulfate crystals are then added to water, the crystals turns blue and heat is given off
- This backward / reverse reaction is exothermic
hydrated copper(II) sulfate ⇌ anhydrous copper(II) sulfate + water
The forward reaction is exothermic and the reverse reaction is endothermic
Examiner Tip
Make sure you know the terms anhydrous, hydrated and water of crystallisation.
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