GCSE Chemistry Revision — Reversible Reactions
Revise Reversible Reactions for GCSE Chemistry with a topic explanation, worked example and common mistakes. Check the board notes for specification differences.
At a glance
- What StudyVector is
- An exam-practice platform with board-aligned questions, explanations, and adaptive next steps.
- This topic
- Reversible Reactions in GCSE Chemistry: explanation, examples, and practice links on this page.
- Who it’s for
- Students revising GCSE Chemistry for UK exams.
- Exam boards
- Check your course page and the topic board notes for supported specifications.
- Free plan
- Sign up free to use tutor paths and feedback on your answers. Free access is Free daily revision · No card required. Pricing
- What makes it different
- Syllabus-shaped practice and progress tracking—not generic AI answers.
This page includes a topic explanation and a worked example. Check your course for current practice coverage.
Next in this topic area
Next step: Dynamic Equilibrium
Continue in the same course — structured practice and explanations on StudyVector.
Go to Dynamic EquilibriumTopic explanation
What 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 examples
Worked 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.
Practise this topic
Start with low-focus cards for Reversible Reactions, then move into full exam-style practice when you want the heavier session.
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
Check the available question sets for Reversible Reactions. Use your course and exam board to confirm which practice is relevant.
Reversible Reactions exam questionsGet help with Reversible Reactions
Get a personalised explanation for Reversible Reactions from the StudyVector tutor. Ask follow-up questions and work through problems with step-by-step support.
Open tutorSave your progress in Reversible Reactions
Start a free account for low-focus question cards, feedback and Play routes across available topics. Free daily limits apply; no card required.
Continue your revision
A public question for Reversible Reactions is still being reviewed. Your course page shows the topics currently available for practice.
Continue with Reversible Reactions
Create a free account to keep your course choice and save your practice progress.
Start free low-focus cardsAlready have an account? Log in
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.