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Chapter 14 Terms

20 terms throughout chapter 14

TermDefinition
Reaction Rate The speed at which a chemical reaction occurs
Chemical Kinetics The area of chemistry concerned with the speeds, or rates, of reactions
Instantaneous rate The rate at a particular instant during the reaction
Rate law The rate depends on reactant concentrations
Rate constant Constant K
Reaction orders The exponents m and n
Overall reaction order The sum of the orders with respect to each reactant represented in the rate law
First order reaction On whose rate depends on the concentration of a single reactant to the first power
Second order reaction On whose rate depends either on a reactant concentration raised to the second power or On the concentration of two reactants each raised to the first power
Zero order reaction One in which the rate of disappearance of A is independent of [A]
Half life The time required for the concentration of a reactant to reach half its initial value
Activation energy The minimum energy required to initiate a chemical reaction
Activated complex or the transition state The difference between the energy of the starting molecule and the highest energy along the reaction pathway is the activation energy
Arrhenius equation k=Ae^-Esuba/RT
Frequency factor Related to the frequency of collisions and the probability that the collisions are favorable oriented for reaction.
Elementary reactons Both reactions occur in a single event of step
Molecularity The number of molecules that participate as reactants in an elementary reaction
Unimolecular A single molecule is involved
Bimolecular Reactions involving the collision of two reactant molecules
Termolecular Elementary reactions involving the simultaneous collision of three molecules
Reaction mechanism The steps by which a reaction occurs
Created by: Trace Villbrandt
 

 



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