This definitions covers Key Definitions 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 7 of 14 in this topic. Make sure you can use the exact wording confidently, because definition marks are often lost through vague language.
📖 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.
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.