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Reversible Reactions (AQA GCSE Chemistry: Combined Science)
Revision Note
Reversible reactions
What are reversible reactions?
- Some reactions go to completion, where the reactants are used up to form the product molecules and the reaction stops when all of the reactants are used up
A + B → C + D
- In reversible reactions, the product molecules can themselves react with each other or decompose and form the reactant molecules again
- It is said that the reaction can occur in both directions:
- The forward reaction (which forms the products)
A + B → C + D
-
- The reverse direction (which forms the reactants)
C + D → A + B
- When writing chemical equations for reversible reactions, two arrows are used to indicate the forward and reverse reactions
- Each one is drawn with just half an arrowhead – the top one points to the right, and the bottom one points to the left: ⇌
A + B C + D
- The direction a reversible reaction takes can be changed by changing the reaction conditions
Reversible reaction example
- Heating ammonium chloride produces ammonia and hydrogen chloride gases
- This is an endothermic process as energy is provided for the reaction
NH4Cl (s) → NH3 (g) + HCl (g)
- As the hot gases cool down they recombine to form solid ammonium chloride
- This is an exothermic process
NH3 (g) + HCl (g) → NH4Cl (s)
- So, the reversible reaction is represented like this:
NH4Cl (s) ⇌ NH3 (g) + HCl (g)
Examiner Tip
The reverse reaction may also be called the backwards reaction.
A generic reversible reaction is shown as:
A + B ⇌ C + D
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