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 25 exam-style questions and 16 flashcards. This topic appears less often, but it can still be a useful differentiator on mixed-topic papers. It is section 8 of 14 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and 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)
Practice questions for Rates & Collision Theory
According to collision theory, which of the following must happen for a chemical reaction to take place?
Explain, using collision theory, why increasing the concentration of a reactant solution increases the rate of reaction.
Quick recall flashcards
What are the units for rate?
g/s, cm³/s, or mol/s
What is rate of reaction?
How quickly reactants are used up or products are formed