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by: Sarahjallen

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# KINETICS STUDY GUIDE CH. 13 Chem 120B

Sarahjallen
Cal State Fullerton

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Exam date: Friday, February 19th 2016 Review these topics!
COURSE
General Chemistry 120B
PROF.
Dr. Richard Deming
TYPE
Study Guide
PAGES
2
WORDS
CONCEPTS
kinetics, Chemistry, Chem, CSUF, cal state fullerton, Chem120B
KARMA
50 ?

## 1

1 review
"Can you just teach this course please? lol :)"
Greyson O'Hara

## Popular in Chemistry and Biochemistry

This 2 page Study Guide was uploaded by Sarahjallen on Monday February 15, 2016. The Study Guide belongs to Chem 120B at California State University - Fullerton taught by Dr. Richard Deming in Spring 2016. Since its upload, it has received 42 views. For similar materials see General Chemistry 120B in Chemistry and Biochemistry at California State University - Fullerton.

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## Reviews for KINETICS STUDY GUIDE CH. 13

Can you just teach this course please? lol :)

-Greyson O'Hara

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Date Created: 02/15/16
KINETICS REVIEW CHAPTER 13 CHEM 120B Exam Date: Friday February 19 2016 th Things to Know:  Draw products and reactants on graph of how reaction took place  Find the rate of the reaction  Find rate law including order of the reaction  Be able to calculate half life  Use integrated rate law to calculate k constant  What’s the deal with activation energy & be able to calculate it  Identify catalyst and intermediates  Mechanisms Rate= Change∈Molecules The rate of a Reaction is calculated by Change∈time also known as the slope. Ex. 2N O2→45 O +O 2 2 −1 1 1 rate= (−32 )+ (+64 ) (16) 2 4 1 Rate =16 RateLaw=K [N O ] [N O ] [O ]y z 2 5 2 2 Calculate x, y, and x using the comparison of different rates & logs. x y z R1=3.8=K 0.[0 [0]20] [0.10] Ex. x y z R 27.7=K[0.10] [0.20] [0.20] Eventually, once every exponent is calculated you can use one equation to find the K constant. After calculating for the K constant, you have your complete rate law! Zero Order First Order Second Order Linear When… [Concentration vs. Ln[concentration] 1/ [concentration] Time] vs. time vs. time Rate law 0 1 2 [NO] [NO] [NO] Half Life Reaction [A]0 0.693 1 t1= t1= t1= 2 2k 2 k 2 K [A]0 (Decreases over (Constant) (Increases over time) time) Integrate Rate law [A =[A] −kt ln[A]=ln A ]−kt 1 1 0 0 = +kt [A] [ A]0 Activation energy: energy initially needed for a reaction to take place. - Equation with less Activation Energy = high reaction rate/ happens faster - Equation with high Activation Energy = small reaction rate / happens slower Ways to Calculate Activation Energy: −Ea Rt  Activation K=Ae Energy Ea 1 1 ln K= − R T 2 T1) Ea 1 ln K=ln A− R T) *Temp is always measure in Kelvin* Forward Rxn: Exothermic (see above) Reverse Rxn: Endothermic *Higher temp = faster Reaction* Catalyst: lowers activation energy needed which makes the reaction happen sooner. In mechanisms, the rate limiting step is the step where there is a collision of molecules. The reaction rate is determined by this step.

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