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Ma P Chem 11/9, 11/11, 11/13

by: Kayli Antos

Ma P Chem 11/9, 11/11, 11/13 CHEM 345

Marketplace > Towson University > Chemistry > CHEM 345 > Ma P Chem 11 9 11 11 11 13
Kayli Antos
GPA 3.37
Physical Chemistry
Dr. Ma

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About this Document

Chapter:Electrolyte Solutions Chapter: Electrochemistry Topics: Components Of An Electrochemical Cell, Half Reactions, The Cell Diagram, Electrode Potential, Cell Potential Chapter: Chemical Kin...
Physical Chemistry
Dr. Ma
Class Notes
25 ?




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This 2 page Class Notes was uploaded by Kayli Antos on Sunday November 15, 2015. The Class Notes belongs to CHEM 345 at Towson University taught by Dr. Ma in Summer 2015. Since its upload, it has received 15 views. For similar materials see Physical Chemistry in Chemistry at Towson University.


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Date Created: 11/15/15
P Chem Ma Fall 3015 Electrolvte Solutions Salting In Effect Solubility increases with ionic strength Electrochemistgy Components OfAn Electrochemical Cell I 2 electrodes copper and zinc in a Daniell Cell I Electrolyte solution I Salt bridge I A wire connecting the electrodes sometimes also connecting a voltmeter bulb etc Half Reactions I Red 9 Ox ne I Ox ne39 9 Red The Cell Diagram 211501 015040161 lCuS I ll salt bridge I phase boundary I The left side is the anode and the right side is the cathode I Can label aqueous solutions with their concentration I If there s no electrode add Pt or Cgraphite as an inert electrode I Electrons ow from high electrode potential anode to low electrode potential cathode Electrode Potential Ered I Intensive property I The higher reduction potential acts as a cathode I Reduction potentials are relative to a standard hydrogen electrode SHE Cell Potential Ecell Electromotive Force emf 39 Ecell EredCathOd Eredan0d I Reversible electrical work I For a cell reaction AG nFEce11 I Faraday s constant 96485 Cmol I Ecell is measured in Volts I CV J I AG is measured in J mol ForA General Reaction I OfaAbB9cCdD AG AG RTan 39 0 RT agag I Eceu E cell n F nagag Nernst Equatlon I At equilibrium AG 0 so Ecell o and E Ceu In K ForA Half Reaction I Of Zns 9 ZII2aq 2e 2 2 I Ox1dat10n electrode potent1al Ered 271 Zn 2 E red 271 Zn E1nZnZ nF I Reduction electrode potential Ered Zquot2Zn E red Zquot2Zn RT 1 n7 n If Ecelllt0 then AGlto and the reaction is not spontaneous z Chemical Kinetics The study of the rates and mechanisms of chemical reactions Reaction Rate v I The change in concentration per unit time dC a v1M111dm adt bdtcdt ddt


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