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Collision theory, theory used to predict the rates of chemical reactions, particularly for gases. The collision theory is based on the assumption that for a reaction to occur it is necessary for the reacting species (atoms or molecules) to come together or collide with one another.
- The Editors of Encyclopaedia Britannica
Collision theory is a principle of chemistry that predicts the rates of chemical reactions based on the number and energy of collisions between reactant molecules. Learn the formula, derivation, and quantitative insights of collision theory for gas-phase and solution reactions.
Feb 13, 2023 · Learn how collision theory explains the rates and mechanisms of chemical reactions. Find out what factors affect the frequency, energy and orientation of collisions, and how they relate to reaction orders and kinetics.
Collision theory states that reactants must collide properly to produce chemical change. Learn how to increase collisions and reaction rates by changing concentration, temperature, pressure, states of matter and catalysts.
Collision theory explains why different reactions occur at different rates, and suggests ways to change the rate of a reaction. Collision theory states that for a chemical reaction to occur, the reacting particles must collide with one another.
Sep 12, 2022 · Collision theory provides a simple but effective explanation for the effect of many experimental parameters on reaction rates. The Arrhenius equation describes the relation between a reaction’s rate constant and its activation energy, temperature, and dependence on collision orientation.
Learn about the collision theory of chemical reactions, which explains how molecules collide and react to form new substances. This web page is part of a free textbook on chemistry by OpenStax, a nonprofit organization.
