Rates of ReactionKey Facts
Key Facts: Rates of Reaction
Part of Rates & Collision Theory — GCSE Chemistry
This key facts covers Key Facts: Rates of Reaction within Rates & Collision Theory for GCSE Chemistry. Revise Rates & Collision Theory in Rates of Reaction for GCSE Chemistry with 20 exam-style questions and 16 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 8 of 13 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 8 of 13
Practice
20 questions
Recall
16 flashcards
📌 Key Facts: Rates of Reaction
- Rate of reaction = how quickly reactants are used up or products are formed
- Collision theory: Reactions only happen when particles collide with enough energy
- Activation energy (Ea) = minimum energy needed for a reaction to occur
- Successful collision = collision with energy ≥ Ea AND correct orientation
- Faster reaction = more successful collisions per second
- On a graph: Steeper gradient = faster rate
- Horizontal line on graph = reaction has finished
- Same final amount = same total product (if same amount of reactant used)