CHEM 110 Lecture Notes - Lecture 16: Equilibrium Constant, Collision Theory, Activation Energy
Document Summary
The rate at which reactants are consumed or products are produced in a chemical reaction. For a reaction to occur: reactant particles must collide, collision must have a certain minimum amount of energy: activation energy, reactants may require a specific orientation. Start with reactants with a certain potential energy per (average pe of all the reactants) End with products with a different potential energy pep (average pe of all the products) In between: for reaction to occur the activation energy must be obtained. Exothermic reaction: energy is released during a chemical reaction. The pe of the products is lower than the pe of the reactants. Endothermic reaction: energy is absorbed during the chemical reaction. The pe of the products is higher than the pe of the reactants. Reactant concentration increase the concentration of reactants, increase the reaction rate: more particles, greater chance of collision.