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CAS CH 131 (61)
Lecture

Electrochemistry

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Department
Chemistry
Course
CAS CH 131
Professor
Andrei Lapets
Semester
Fall

Description
Electrochemistry 12/11/2012 ***LOOK AT 17.4 AND 17.6****** Electrochemistry energy released by a spontaneous reaction is converted into electricity or electricity becomes energy put into a reaction Always a redox reaction reduction = gaining an electron oxidation = losing an electron oxidizing agent = gains electron and causes oxidation reducing agent = loses electron and causes reduction Mg  (s)HCl  ▯ M(aq) 2(aq)+ H 2(g) H goes from +1 to 0 Mg goes from 0 to +2 Mg  is the reducing agent HCl is the oxidizing agent Electrochemical cell Zn  + Cu  ▯ Zn 2 + Cu 0 Cu reduces from 2+ to 0 Zn oxidizes from 0 to 2+ salt bridge made of KCl anode oxidizes, cathode reduces, so electrons flow through wires from Zn to Cu ­ 2+ Cl balances Zn  otherwise reaction would stop K  balances right side because losing Cu 2+ spontaneous reaction 2+ 2+ Zn (s) (1 M)||Cu (1 M)|Cu (s) single line is a phase boundary, double line is separation needs to stay separate otherwise reaction would work but would stop a lot sooner E = 1.1 V opposite reaction: Zn  + Cu  ▯ Zn  + Cu 0 +2 ΔG > 0, not spontaneous called electrolysis where a battery is needed E = ­1.1 V Faraday’s Law (1) the mass of a given substance produced or consumed is proportional to the quantity of electrical charge  passed (2) the number of moles of product formed by an electrical current is stoichiometrically equivalent to the  number of moles of electrons supplied +2 ­ 0 Cu  + 2e ▯ Cu ­ 0 2 mol e = 1 mol Cu ­19 charge of electrons: 1.60217646x10  C 23 ­19 charge on a mole of electrons: (6.02x10 )(1.6x10 ) = 96485.34 C/mol = Faraday’s constant +1 0 0 +2 2Ag  + Cu  ▯ 2Ag  + Cu 0 current of 0.5 A passed through cell for 101 minut
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