GCSE Chemistry (AQA)

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Reversible Reactions

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Reversible reactions and dynamic equilibrium Reversible reactions

Reversible Reactions

6:03 Reversible Reactions
Spec 4.6.2.1 4.6.2.2
Previous The Haber Process: Equilibrium
  • Arrows indicate the direction of a chemical reaction from reactants to products.
  • Burning wood produces smoke and ash, represented by the equation: Wood + Oxygen ��� Carbon Dioxide + Water Vapor + Ash.
  • In this reaction, wood and oxygen are reactants, and carbon dioxide, water vapor, and ash are products.
  • The reaction is irreversible; products cannot revert to reactants.
  • Some reactions are reversible, where products can revert to original reactants.
  • Example: Heating ammonium chloride decomposes it into ammonia and hydrogen chloride, which can recombine upon cooling.
  • Reversible reactions are shown with a two-way arrow in chemical equations.
  • The direction of reversible reactions can change with conditions, such as temperature.
  • Reversible reactions can be endothermic in one direction and exothermic in the opposite.
  • Example: Heating ammonium chloride is endothermic; cooling products to reform ammonium chloride is exothermic.
  • The energy transferred is equal in both directions of a reversible reaction.
  • Example: Hydrated copper sulfate can be dehydrated to anhydrous copper sulfate and reversed by adding water.
  • Recognize reversible reactions by their symbol and understand how conditions affect direction.
  • In reversible reactions, if one direction is exothermic, the opposite is endothermic, with equal energy transfer.

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