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Final

CHE102 Study Guide - Final Guide: Elementary Reaction, Reduction Potential, Standard Hydrogen Electrode


Department
Chemical Engineering
Course Code
CHE102
Professor
Perry Chou
Study Guide
Final

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o Standard hydrogen electrode is the basis half-cell reactions are compared to when
determining their standard reduction potential (concentration is 1M)
o Reduction potentials also depend on the concentration of the half-cell
o In these cases we apply the Nernst equation
  

   





 
o If >0 then the rxn is spontaneous, and if <0 then the rxn is non-spontaneous
o Concentration cells are cells in which the same half cell is acts anode and cathode, the
only difference is concentration
o Faraday’s law relates the charge passed through a cell to the mass consumed/produced
  


o Electrolysis
Is the same as a galvanic cell except an electrolytic cells standard cell potential is
negative, and therefore not spontaneous
Needs an external battery to drive the reaction
Using Faraday’s la e can relate the charge used to drie the reaction ith the
amount of material produced/consumed in the reaction
Chemical Kinetics
o Expressing rxn rates for example    
(Rate of reaction )=
(Rate of reaction )=(rate of reaction )
  



 

reactants are (-), products are (+)
o Rate Laws relates rate to the [] of reactants (A and B) and temperature
  
The best Table to put on your cheat sheet ever
Order of rxn
Zero
First
Second
Rate Law
Rate=k
Rate=k[A]
Rate=k[A]2
Integrated Rate Law
[A]=[Ainitial]-kt
ln[A]-ln[Ainitial]=-kt
1/[A]-1/[Ainitial]=kt
Units of k
M/s
1/s
1/(M*s)
Linear plot
[A] vs t
ln[A] vs t
1/[A] vs t
slope
-k
-k
K
Half life
t1/2=1/2[Ainitial]k
t1/2=0.693/k
t1/2=1/([Ainitial]k)
o Arrhenius Law (used for questions relating to activation energy of a reaction)
 

 
K is rate constant, A is a constant factor depending on the reaction, and Ea is
activation energy
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find more resources at oneclass.com
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