Common Misconceptions
Part of Reversible Reactions — GCSE Chemistry
This common misconceptions covers Common Misconceptions within Reversible Reactions for GCSE Chemistry. Revise Reversible Reactions in Rates of Reaction for GCSE Chemistry with 20 exam-style questions and 12 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 8 of 12 in this topic. Use this common misconceptions to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 8 of 12
Practice
20 questions
Recall
12 flashcards
⚠️ Common Misconceptions
Misconception 1: "Reversible means the reaction goes backwards"
A reversible reaction does not simply "go backwards" — both directions happen simultaneously. Even as products are forming, some are reacting together to reform reactants. The ⇌ symbol explicitly shows that both the forward and backward reactions are occurring at the same time. The net direction just depends on which reaction is currently faster.
Misconception 2: "Reversible reactions reach 100% products eventually"
In a closed system, a reversible reaction never reaches 100% conversion. The system reaches a state of dynamic equilibrium where both forward and backward rates are equal. This is why industrial processes like the Haber process must recycle unreacted gases — you can never convert all the reactants in one pass.
Misconception 3: "The energy values are different for forward and backward reactions"
The energy released in the exothermic direction always equals the energy absorbed in the endothermic direction. If the forward reaction releases 100 kJ/mol, the backward reaction absorbs exactly 100 kJ/mol. This follows from conservation of energy.