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Use the tabulated electrode potentials to calculate K for the oxidation of iron by H++ (at 25°C): 2Fe(s)+6H+(aq)→2Fe3

Use the tabulated electrode potentials to calculate K for the oxidation of iron by H++ (at 25°C): 2Fe(s)+6H+(aq)→2Fe3

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.72QP: What is the standard cell potential you would obtain from a cell at 25C using an electrode in which...
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Use the tabulated electrode potentials to calculate K for the oxidation of iron by H++ (at 25°C):

2Fe(s)+6H+(aq)→2Fe3+(aq)+3H2(g)

TABLE 18.1 Standard Reduction Potentials at 25°C E° Reduction Half-Reaction (V) 2 F (aq) Stronger oxidizing agent F2(g) + H2O;(aq) + 2 H*(aq) + 2 e- MnO, (aq) + 8 H*(aq) + 5 e Cl2(8) + 2 e- Cr,0, (aq) + 14 H*(aq) + 6 e O:(8) + 4 H*(aq) + 4 e- Br2(1) + 2 e Ag*(aq) + e Fe*(aq) + e Oz(g) + 2 H*(aq) + 2 e I2(s) + 2 e- O:(g) + 2 H,O(1) + 4 e- Cu2*(aq) + 2 e Sn*(aq) + 2 e 2 e 2.87 Weaker reducing agent 2 H;O(I) 1.78 → Mn2 (aq) + 4 H,O(1) →2 CI(aq) →2 Cr* (aq) + 7 H;O() → 2 H;O(I) →2 Br (aq) → Ag(s) Fe2*(aq) (bv)O°H 2 1 (aq) → 4 OH"(aq) 1.51 1.36 1.33 1.23 1.09 0.80 0.77 0.70 0.54 0.40 Cu(s) 0.34 • Sn²*(aq) 0.15 2 H*(aq) + 2 e- Pb2*(aq) + 2e Ni2*(aq) Pb(s) Ni(s) → Cd(s) → Fe(s) -0.13 + 2 e Cd2*(aq) + 2 e Fe2*(aq) + 2 e Zn2*(aq) + 2 e- 2 H,O() + 2 e Al"(aq) + 3 e Mg*(aq) + 2e Na*(aq) + e- Li*(aq) + e -0.26 -0.40 -0.45 >Zn(s) → H2(g) + 2 OH(aq) → Al(s) → Mg(s) → Na(s) → Li(s) -0.76 -0.83 -1.66 -2.37 Stronger reducing agent Weaker -2.71 oxidizing agent -3.04
Transcribed Image Text:TABLE 18.1 Standard Reduction Potentials at 25°C E° Reduction Half-Reaction (V) 2 F (aq) Stronger oxidizing agent F2(g) + H2O;(aq) + 2 H*(aq) + 2 e- MnO, (aq) + 8 H*(aq) + 5 e Cl2(8) + 2 e- Cr,0, (aq) + 14 H*(aq) + 6 e O:(8) + 4 H*(aq) + 4 e- Br2(1) + 2 e Ag*(aq) + e Fe*(aq) + e Oz(g) + 2 H*(aq) + 2 e I2(s) + 2 e- O:(g) + 2 H,O(1) + 4 e- Cu2*(aq) + 2 e Sn*(aq) + 2 e 2 e 2.87 Weaker reducing agent 2 H;O(I) 1.78 → Mn2 (aq) + 4 H,O(1) →2 CI(aq) →2 Cr* (aq) + 7 H;O() → 2 H;O(I) →2 Br (aq) → Ag(s) Fe2*(aq) (bv)O°H 2 1 (aq) → 4 OH"(aq) 1.51 1.36 1.33 1.23 1.09 0.80 0.77 0.70 0.54 0.40 Cu(s) 0.34 • Sn²*(aq) 0.15 2 H*(aq) + 2 e- Pb2*(aq) + 2e Ni2*(aq) Pb(s) Ni(s) → Cd(s) → Fe(s) -0.13 + 2 e Cd2*(aq) + 2 e Fe2*(aq) + 2 e Zn2*(aq) + 2 e- 2 H,O() + 2 e Al"(aq) + 3 e Mg*(aq) + 2e Na*(aq) + e- Li*(aq) + e -0.26 -0.40 -0.45 >Zn(s) → H2(g) + 2 OH(aq) → Al(s) → Mg(s) → Na(s) → Li(s) -0.76 -0.83 -1.66 -2.37 Stronger reducing agent Weaker -2.71 oxidizing agent -3.04
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