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Chapter 18 Vocabulary: Reaction Rates and Equilibrium

activated complex The arrangement of atoms at the peak of the activation energy barrier.
activation energy (Ea) The minimum energy colliding particles must have in order to react.
transition state This is what the activated complex is sometimes called.
Collision theory says that atoms, ions, and molecules can form a chemical bond when they collide, provided the particles have enough kinetic energy.
catalyst A substance that increases the rate of a reaction without being used up itself in the reaction.
reversible reaction The reactions in both directions occur simultaneously.
chemical equilibrium This is when the forard and the reverse reactions are taking place at the same time.
Le Chatelier's principle If a stress is applied to a system in a dynamic equilibrium, the system changes to relieve the stress.
spontaneous reaction Naturally favor the formation of products at the specified conditions.
nonspontaneous reaction Do not favor the formation of products at the specified conditions.
equilibrium constant (Keq) The ratio of product concentrations to reactant concentrations, with each concentration raised to a power given by the number of moles of that substance in the balanced chemical equation.
entropy Of a liquid or solid substance at 25 degrees celcius and 101.3 kPa is designated S^o
Reaction Rate Speed at which a chemical reaction proceeds, in terms of amount of product formed or amount of reactant consumed per unit of time.
solubility product constant (Ksp) Is equal to the product of the concentration terms each raised to the power of the coefficient of the substance in the dissociation equation.
enthalpy The amount of heat that a substance has at a given temperature or pressure.
potential energy diagram shows how energy changes during the course of a chemical reaction.
Created by: KellyBeck