Ch 11 Z - Electrochemistry for posting

Ch 11 Z - Electrochemistry for posting -...

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Unformatted text preview: Oxidation-reduction reactions • Oxidation: Loss of electrons (consider oxidation of Fe to Fe3+ as in Fe2O3 , rust) • Reduction: Gain of electrons (Reduction of formal charge) OIL RIG 2Ag(s) + Cu2+ 2Ag+ + Cu(s) 2e- oxidized reduced Consider the reaction between Zn and Cu2+ Zn + Cu2+ ⇆ Zn2+ + Cu This will take place spontaneously in solution (i.e., ∆ Go <0, Keq > 1) C u 2 + C u Z n 2 + Z n Z n Z n Z n Z n Z n Z n Z n Z n Z n Z n Z Z n Z n Z n Z n Z n Z n …electron transfer… OIL RIG Let’s separate the reactants Zn Cu Cu2+ Zn2+ Anode (oxidation) Cathode (reduction) Zn(s) Zn2+ +2e Cu2+ +2e Cu(s) Cu2+ Zn2+ Zn(s)+ Cu2+ +2e T Zn2+ Cu(s) +2e Zn(s)+ Cu2+ Zn2+ Cu(s) Cell potential (volts) A few other images showing connections Voltmeter or potentiometer used to measure “driving force”, i.e., electromotive force or emf. Expressed in units of volts (1 V=1 J/coulomb) Conventions : O xidation at a node R eduction at c athode Anode is on the left side Cathode is on the right Analogy to water in hose : Pressure = emf (volts) Flow = current (amps) Consider the oxidation-reduction...
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This note was uploaded on 04/04/2010 for the course CH 52460 taught by Professor Holcombe during the Spring '10 term at University of Texas.

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Ch 11 Z - Electrochemistry for posting -...

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