Common Misconceptions
Part of Exothermic Reactions — GCSE Chemistry
This common misconceptions covers Common Misconceptions within Exothermic Reactions for GCSE Chemistry. Revise Exothermic Reactions in Energy Changes for GCSE Chemistry with 20 exam-style questions and 14 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
14 flashcards
⚠️ Common Misconceptions
Misconception 1: "Exothermic means the products are hot"
Being exothermic does not mean the products themselves are hot — it means energy is transferred TO THE SURROUNDINGS, raising their temperature. The surroundings get hotter, not the products themselves. Rusting iron is exothermic but you can touch rust without getting burned — the energy is released very slowly.
Misconception 2: "Exothermic reactions create energy"
Energy is NEVER created or destroyed — it is transferred. In an exothermic reaction, energy is transferred from the chemical bonds of the reactants to the surroundings as heat. The law of conservation of energy always applies.
Misconception 3: "All reactions that get hot are exothermic — cold means endothermic"
The temperature change of the surroundings (including the solution) tells you whether a reaction is exothermic or endothermic. If the solution temperature RISES → exothermic. If it FALLS → endothermic. The key word is surroundings — not the reaction system itself.