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Redox reaction Experimental Theoretical Cell potential Cell potential 1. Zinc-Copper 0.75 2. Iron-copper 0.62 3. Zinc-iron 0.25 Theoretical cell potential E= E' cell - RT/nF InQ., Q= [product]/[reagent] Concentrations of product and reagent are 1M, Ln1%30, So RT/nF InQ = 0 Then, Theoretical cell potential E cell = E°cell E° cell = E redox- E oxidation %3D You need to identify the anode (oxidize, donate e) and cathode (reduce, gain e) Anode comes first (on the left), cathode come on the right reaction that occurs in the anode compartment. For the Zn/Cu Cell, the standard cell potential, E" E Pa 034 0.76 - 1.10 V. For galvanic cells, E' is always positive. Half reaction E (V) Cu + 2e Cu 034 cathat

Redox reaction Experimental Theoretical Cell potential Cell potential 1. Zinc-Copper 0.75 2. Iron-copper 0.62 3. Zinc-iron 0.25 Theoretical cell potential E= E' cell - RT/nF InQ., Q= [product]/[reagent] Concentrations of product and reagent are 1M, Ln1%30, So RT/nF InQ = 0 Then, Theoretical cell potential E cell = E°cell E° cell = E redox- E oxidation %3D You need to identify the anode (oxidize, donate e) and cathode (reduce, gain e) Anode comes first (on the left), cathode come on the right reaction that occurs in the anode compartment. For the Zn/Cu Cell, the standard cell potential, E" E Pa 034 0.76 - 1.10 V. For galvanic cells, E' is always positive. Half reaction E (V) Cu + 2e Cu 034 cathat

Chemistry
Chemistry
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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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Part 1 Redox reaction Experimental Theoretical Cell potential Cell potential 1. Zinc-Copper 0.75 2. Iron-copper 0.62 3. Zinc-iron 0.25 Theoretical cell potential E= E cell – RT/nF InQ., Q= [product]/[reagent] Concentrations of product and reagent are 1M, Ln1=0, So RT/nF InQ = 0 Then, Theoretical cell potential E cell = E°cell E° cell = E redox - E oxidation %3D You need to identify the anode (oxidize, donate e) and cathode (reduce, gain e) Anode comes first (on the left), cathode come on the right reaction that dccurs in the anode compartment. For the Zn/Cu Cell, the standard cell potential, E E Pa 034 + 0.76 = 1.10 V. For galvanic cells, E is always positive. Half reaction E* (V) Cut + 2e Cu 034 Fel + 2e → Fe 0.44 Zn + 2e Zn 0.76 Table 16.1: Standard reduction potentials at 25 "C E° values are on table 16.1 page 127 thant
Transcribed Image Text:Part 1 Redox reaction Experimental Theoretical Cell potential Cell potential 1. Zinc-Copper 0.75 2. Iron-copper 0.62 3. Zinc-iron 0.25 Theoretical cell potential E= E cell – RT/nF InQ., Q= [product]/[reagent] Concentrations of product and reagent are 1M, Ln1=0, So RT/nF InQ = 0 Then, Theoretical cell potential E cell = E°cell E° cell = E redox - E oxidation %3D You need to identify the anode (oxidize, donate e) and cathode (reduce, gain e) Anode comes first (on the left), cathode come on the right reaction that dccurs in the anode compartment. For the Zn/Cu Cell, the standard cell potential, E E Pa 034 + 0.76 = 1.10 V. For galvanic cells, E is always positive. Half reaction E* (V) Cut + 2e Cu 034 Fel + 2e → Fe 0.44 Zn + 2e Zn 0.76 Table 16.1: Standard reduction potentials at 25 "C E° values are on table 16.1 page 127 thant
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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