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Redox Reaction Experimental Cell Potential Theoretical Cell Potential Zn(0.1M)-Cu(1M) 0.95 Zn(0.1M)-Zn(1M) 0.08 Cu(0.1M)-Cu(1M) 0.019

Redox Reaction Experimental Cell Potential Theoretical Cell Potential Zn(0.1M)-Cu(1M) 0.95 Zn(0.1M)-Zn(1M) 0.08 Cu(0.1M)-Cu(1M) 0.019

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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We are given information about variables in Nernst equation and concentration of ions. We need to determine the theoretical cell potential. Please help.
Redox Reaction Experimental Cell Potential Theoretical Cell Potential Zp Zn(0.1M)-Cu(1M) 0.95 Zn(0.1M)-Zn(1M) 0.08 Cu(0.1M)-Cu(1M) 0.019
Transcribed Image Text:Redox Reaction Experimental Cell Potential Theoretical Cell Potential Zp Zn(0.1M)-Cu(1M) 0.95 Zn(0.1M)-Zn(1M) 0.08 Cu(0.1M)-Cu(1M) 0.019
reactions appears on the list as it occurs. The other half-reaction occurs as oxidation and its reverse is on the list. The oxidation potential is the negative of the listed reduction potential. 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 cell potential, E°cell = E°red + E°ox = 0.34 + 0.76 = 1.10 V. For galvanic cells, E°cell is always positive. galvantc cell Half reaction E° (V) Cu2+ + 2e → Cu 0.34 Fe2+ + 2e → Fe -0.44 Zn2+ + 2e → Zn -0.76 Table 16.1: Standard reduction potentials at 25 °C Nernst equation The Nernst equation allows us to determine the cell potential at non-standard conditions. lues RT Ecell = E°cell -InQ, where E°cell is the standard cell potential, the gas constant (8.314 J/mol K), T the temperature in K, F the Faraday constant (96485 C/mol), and Q the reaction quotient. the iron and coper In this laboratory experiment, you will study galvanic cells. You will construct different cells, measure their cell potentials, and study the effect of concentration and temperature on 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°. Inotsb Element/ion AH;° (kJ/mol) AG (kJ/mol) S° (J/mol K)oy Cu(s) Cu2"(aq) Fe(s) Fe2 (aq) Zn(s) 33.2 -99.6 phise adhitN 64.8 65.5 27.3 0. -78.9 -137.7 -89.1 26ulsv s 41.6 0. -112.1 Zn*(aq) -153.9 -147.2 Table 16.2: Thermodynamic Data for 25 °C Experiment 16
Transcribed Image Text:reactions appears on the list as it occurs. The other half-reaction occurs as oxidation and its reverse is on the list. The oxidation potential is the negative of the listed reduction potential. 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 cell potential, E°cell = E°red + E°ox = 0.34 + 0.76 = 1.10 V. For galvanic cells, E°cell is always positive. galvantc cell Half reaction E° (V) Cu2+ + 2e → Cu 0.34 Fe2+ + 2e → Fe -0.44 Zn2+ + 2e → Zn -0.76 Table 16.1: Standard reduction potentials at 25 °C Nernst equation The Nernst equation allows us to determine the cell potential at non-standard conditions. lues RT Ecell = E°cell -InQ, where E°cell is the standard cell potential, the gas constant (8.314 J/mol K), T the temperature in K, F the Faraday constant (96485 C/mol), and Q the reaction quotient. the iron and coper In this laboratory experiment, you will study galvanic cells. You will construct different cells, measure their cell potentials, and study the effect of concentration and temperature on 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°. Inotsb Element/ion AH;° (kJ/mol) AG (kJ/mol) S° (J/mol K)oy Cu(s) Cu2"(aq) Fe(s) Fe2 (aq) Zn(s) 33.2 -99.6 phise adhitN 64.8 65.5 27.3 0. -78.9 -137.7 -89.1 26ulsv s 41.6 0. -112.1 Zn*(aq) -153.9 -147.2 Table 16.2: Thermodynamic Data for 25 °C Experiment 16
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