IMG_0001_NEW_0026_001

IMG_0001_NEW_0026_001 - . Reduction half reaction: Ct*(aq)+...

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LECTURE: L,\ .TODAY'S Electrochemistry "The study of the interchange of chemical and electrical enerry" > Reduction-Oxidation (Redox) Reactions (rxns involving the transfer of electrons) -> 2 Processes O the generation of an electric current from a chemical reaction @ the use of electric current to produce chemical change Important applications: . Batteries . Corrosion prevention . Commercial electrolyticprocesses 2 "Electrochemistry" (Chapter 11) l) Galvanic Cells 2) Standard Reduction Potentials 3) Standard Hydrogen Electrode Redox processes For the redox reaction: zr{A> + Ct}*(aq) -+ Zr**(aq1 + Cri'1s) . Oxidation half reaction: Zn(s) -+ Z**(aq) + 2e- (loss of electrons) + Increase oxidation number
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Unformatted text preview: . Reduction half reaction: Ct*(aq)+ 2e-+ Cu(s) (gainof electrons) + Reduced oxidation number . Spontaneous reaction: Put Ztncmetalrn CrP* solution -+ coppermetal Zn: reducing agent (reduces Cu2*) Cu2*: oxidizing agent (oxidizes Zn) 1) 2) Generating Gurrent Separate two half reactions\-, Current Link metals (electrodes) J - @- flow) Znmetal ZnSOu(aq) solution-+Znz* + SO42- (1M) Oxidation occurs at Anode (Zn electrode) Zn(s) -+ Zr*+(aq) + 2e-Cu Metal CuSOo(aq) solution-+ Cu2+ + SO42- (lM) Reduction occurs at Cathode (Cu electrode) A**@q) + 2e- -+ Cu(s) Electrons flow from anode + cathode But only for an instant! Charge builds up on each side...
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