Reversible Reactions — GCSE Chemistry Revision
Revise Reversible Reactions for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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Go to Dynamic EquilibriumWhat is Reversible Reactions?
A reversible reaction is a chemical reaction that can proceed in both the forward and reverse directions. The direction of the reaction can be changed by altering the conditions. A special arrow (⇌) is used to represent a reversible reaction in a chemical equation.
Board notes: Reversible reactions are a key concept for all exam boards, setting the stage for understanding chemical equilibrium. You need to be able to recognise and write equations for reversible reactions.
Step-by-step explanationWorked example
The reaction between nitrogen and hydrogen to form ammonia in the Haber process is reversible: N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Ammonia can also decompose back into nitrogen and hydrogen.
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Common mistakes
- 1Thinking that the reaction stops once it reaches equilibrium. The forward and reverse reactions continue to happen, but at the same rate.
- 2Confusing the symbol for a reversible reaction (⇌) with other types of arrows.
- 3Assuming that at equilibrium, the concentrations of reactants and products are equal. They are simply constant.
Reversible Reactions exam questions
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Reversible Reactions
Core concept
A reversible reaction is a chemical reaction that can proceed in both the forward and reverse directions. The direction of the reaction can be changed by altering the conditions. A special arrow (⇌) i…
Frequently asked questions
What does the double arrow (⇌) mean?
The double arrow indicates that the reaction is reversible, meaning it can go both forwards (reactants to products) and backwards (products to reactants) at the same time.
Can all reactions be reversed?
In theory, all reactions are reversible to some extent, but in many cases, the reverse reaction is so slow or energetically unfavourable that the reaction is considered irreversible for practical purposes, like combustion.