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Week 1 Notes

by: Josilynn Stokes

Week 1 Notes Chem 122A

Josilynn Stokes

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About this Document

These notes is what we covered in the first week of school.
Gen Chemistry 2
Marykay Orgill
Class Notes
reaction, Rates




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This 2 page Class Notes was uploaded by Josilynn Stokes on Tuesday September 6, 2016. The Class Notes belongs to Chem 122A at University of Nevada - Las Vegas taught by Marykay Orgill in Fall 2016. Since its upload, it has received 87 views. For similar materials see Gen Chemistry 2 in Chemistry at University of Nevada - Las Vegas.


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Date Created: 09/06/16
Chapter 14: Chemical Kinetics  Kinetics is the study of reaction rates and how much  of the concentration of the product changes with time   Products concentration tends to increase while  Reactants concentration tends to increase  Concentration is shown with “[]”   Collision theory   Reactant particles must collide   Reactant must come into contact in the proper  orientation (has to be lined up the right way)  Reactants must have a sufficient amount of energy to  react   Surface Area and the effect on reaction rate   Ex. If there was an iron nail in a bottle of oxygen the  reaction would occur slowly because it is only reacting with the outer layer of molecules. If the iron nail was  replaced with iron wool the reaction rate is higher  because there is more molecules throughout the wool.  Orientation and the effect on reaction rates   The second part of the collision theory says that  molecules have to be in the right orientation to react  There are certain enzymes that aid in this process.  Enzymes hold the molecule in a certain orientation so  that other molecules can collide and react.  Energy and the effect on reaction rate  Higher temperature increases the energy the molecule  has. The higher the energy the faster the molecule  moves. The faster the molecule moves the higher  chance of a collision. Higher chance of collision  means there is a higher chance of having an effective  collision.  Rate is how much a quantity changes in a given time  period  Over time a reaction rate typically slows. This is  because the amount of reactant decreases over  time. When the amount of reactant decreases, the  probability of a proper collision will decrease.  Thus, having a decreased probability of an  effective collision.   Reaction order: the bigger the order of reaction  the more reactant effects the rate (this comes  from the experiment) th  0  order= [A] vs. time  1  order= ln[A] vs. time   2  order= 1/[A] vs. time  


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