This definitions covers Key Definitions 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 7 of 13 in this topic. Make sure you can use the exact wording confidently, because definition marks are often lost through vague language.
Topic position
Section 7 of 13
Practice
20 questions
Recall
16 flashcards
📖 Key Definitions
Rate of reaction: A measure of how quickly reactants are converted into products, calculated as the amount of reactant used or product formed divided by time.
Collision theory: The model that states a reaction occurs when particles collide with energy greater than or equal to the activation energy and with the correct orientation.
Activation energy (Ea): The minimum energy that colliding particles must possess for a reaction to occur. It is the energy needed to break existing bonds in the reactants.
Successful collision: A collision between reactant particles that results in a reaction — one with sufficient energy and correct orientation.