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Kinetics key terms
Use these key terms for Kinetics in AQA Chemistry 7405. The page is built from approved learning objectives for this topic and links back to the wider unit, topic hub, and related revision assets.
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key terms
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Topic
Kinetics
Key terms
activation energy
The minimum energy required for a chemical reaction to occur. In Collision theory, activation energy is used to explain define activation energy with A-Level Chemistry precision.
collision theory
A theory that states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.
collision frequency
The number of collisions that occur per unit time between reacting particles. In Collision theory, collision frequency is used to explain explain why most collisions do not lead to reaction with A-Level Chemistry precision.
activation energy
The minimum energy required for a reaction to occur when particles collide. In Collision theory, activation energy is used to explain explain why most collisions do not lead to reaction with A-Level Chemistry precision.
collision frequency
The number of collisions that occur per unit time between reacting particles. In Collision theory, collision frequency is used to explain use collision frequency and energy to explain reaction rate with A-Level Chemistry precision.
activation energy
The minimum energy required for a reaction to occur when particles collide. In Collision theory, activation energy is used to explain use collision frequency and energy to explain reaction rate with A-Level Chemistry precision.
Maxwell-Boltzmann distribution
A graphical representation showing the distribution of kinetic energies of particles in a gas at a given temperature.
activation energy
The minimum energy required for a reaction to occur, represented as the peak of the energy barrier in the Maxwell-Boltzmann distribution.
Maxwell-Boltzmann distribution
A statistical distribution that describes the energy distribution of particles in a gas, showing how many particles have a certain energy at a given temperature.
activation energy
The minimum energy required for a chemical reaction to occur, which corresponds to the peak of the energy barrier in a reaction pathway.
activation energy
The minimum energy required for a chemical reaction to occur. In Maxwell-Boltzmann distribution, activation energy is used to explain use the area beyond activation energy to explain rate changes with A-Level Chemistry precision.
Maxwell-Boltzmann distribution
A statistical distribution that describes the energies of particles in a gas at a given temperature.
activation energy
The minimum energy required for a chemical reaction to occur, allowing particles to collide effectively.
Maxwell-Boltzmann distribution
A statistical distribution that describes the energy distribution of particles in a gas, illustrating how temperature affects reaction rates.
collision frequency
The number of collisions that occur per unit time between reacting particles, influencing the rate of reaction.
reaction rate
The speed at which reactants are converted into products in a chemical reaction, often measured in concentration change over time.
activation energy
The minimum energy required for a chemical reaction to occur. In Factors affecting reaction rate, activation energy is used to explain explain how pressure affects gas reaction rate with A-Level Chemistry precision.
collision theory
A theory that states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.
catalyst
A substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with a lower activation energy.
activation energy
The minimum energy required for a chemical reaction to occur, allowing particles to collide and react.
activation energy
The minimum energy required for a chemical reaction to occur. In Factors affecting reaction rate, activation energy is used to explain required practical: investigate how reaction rate changes with temperature with A-Level Chemistry precision.
collision frequency
The number of collisions that occur per unit time between reacting particles. In Factors affecting reaction rate, collision frequency is used to explain required practical: investigate how reaction rate changes with temperature with A-Level Chemistry precision.
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