please show work reactions appears on the list as it occurs. The other half-reaction occurs as oxidation and itsreverse is on the list. The oxidation potential is the negative of the listed reductionpotential. The standard cell potential is the sum of the reduction potential of the half-reaction that occurs in the cathode compartment and the oxidation potential of the half-reaction that occurs in the anode compartment. For the Zn/Cu Cell, the standard cellpotential, E°cell = E°red + E°ox = 0.34 + 0.76 = 1.10 V. For galvanic cells, E°cell is alwayspositive.galvantc cellHalf reactionE° (V)Cu2+ + 2e → Cu0.34Fe2+ + 2e → Fe-0.44Zn2+ + 2e → Zn-0.76Table 16.1: Standard reduction potentials at 25 °CNernst equationThe Nernst equation allows us to determine the cell potential at non-standard conditions.luesRTEcell = E°cell -InQ,where E°cell is the standard cell potential,the gas constant (8.314 J/mol K), T thetemperature in K, F the Faraday constant (96485 C/mol), and Q the reaction quotient.the iron and coperIn this laboratory experiment, you will study galvanic cells. You will construct differentcells, measure their cell potentials, and study the effect of concentration and temperatureon it. To study the temperature dependence, you need the following two equations:AG° = AH° – TAS° and AG° = –NFE°Combine these two equations to derive a relationship between E° and AH° and AS°.InotsbElement/ion AH;° (kJ/mol) AG (kJ/mol) S° (J/mol K)oyCu(s)Cu2"(aq)Fe(s)Fe2 (aq)Zn(s)33.2-99.6phise adhitN64.865.527.30.-78.9-137.7-89.126ulsv s41.60.-112.1Zn*(aq)-153.9-147.2Table 16.2: Thermodynamic Data for 25 °CExperiment 16 Part 2Redox reactionExperimentalTheoreticalCell potentialCell potentiala. Zn(0.1M)-Cu(0.1M)0.92b. Zn(1M)-Cu(0.1M)0.9c. Zn(0.1M)-Cu(1M)0.95d. Zn(0.1M)-Zn(0.1M)0.002e. Zn(0.1M)-Zn(1M)0.08f. Cu(0.1M)-Cu(1M)0.019Theoretical cell potential E = E° cell –RT/nF InQQ = [ product]/[reactant]R= 8.314T= 298.15F=96485n=2 electronE° cell = E° redox – E° oxidation

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Part 2 Redox reaction Experimental Theoretical Cell potential Cell potential a. Zn(0.1M)-Cu(0.1M) 0.92 b. Zn(1M)-Cu(0.1M) 0.9 c. Zn(0.1M)-Cu(1M) 0.95 d. Zn(0.1M)-Zn(0.1M) 0.002 e. Zn(0.1M)-Zn(1M) 0.08 f. Cu(0.1M)-Cu(1M) 0.019 Theoretical cell potential E = E° cell –RT/nF InQ Q = [ product]/[reactant] R= 8.314 T= 298.15 F=96485 n=2 electron E° cell = E redox – E° oxidation

Part 2 Redox reaction Experimental Theoretical Cell potential Cell potential a. Zn(0.1M)-Cu(0.1M) 0.92 b. Zn(1M)-Cu(0.1M) 0.9 c. Zn(0.1M)-Cu(1M) 0.95 d. Zn(0.1M)-Zn(0.1M) 0.002 e. Zn(0.1M)-Zn(1M) 0.08 f. Cu(0.1M)-Cu(1M) 0.019 Theoretical cell potential E = E° cell –RT/nF InQ Q = [ product]/[reactant] R= 8.314 T= 298.15 F=96485 n=2 electron E° cell = E redox – E° oxidation

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.30QAP

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