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Investigate the formation of oxygen gas from a basic solution (formation of O2 from OH-) coupled with the given cathode reaction. Calculate the standard Gibbs energy change of reaction, equilibrium constant (K), and standard electrode potential of the cell. Also, indicate if the redox couple describes a galvanic or electrolytic cell in standard conditions. Use the table shown below. a) Cu^2+ | Cu b) Li^+ | Li

Investigate the formation of oxygen gas from a basic solution (formation of O2 from OH-) coupled with the given cathode reaction. Calculate the standard Gibbs energy change of reaction, equilibrium constant (K), and standard electrode potential of the cell. Also, indicate if the redox couple describes a galvanic or electrolytic cell in standard conditions. Use the table shown below. a) Cu^2+ | Cu b) Li^+ | Li

Physical Chemistry
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter8: Electrochemistry And Ionic Solutions
Section: Chapter Questions
Problem 8.10E: For each of the following reactions, determine the overall balanced electrochemical reaction, its...
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Investigate the formation of oxygen gas from a basic solution (formation of O2 from OH-) coupled with the given cathode reaction. Calculate the standard Gibbs energy change of reaction, equilibrium constant (K), and standard electrode potential of the cell. Also, indicate if the redox couple describes a galvanic or electrolytic cell in standard conditions. Use the table shown below.

a) Cu^2+ | Cu

b) Li^+ | Li

TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E°(V) F-(g) + 2e O3(g) + 2H*(aq) + 2e¯ → 0,(g) + H2O Со" (aq) + e H,O,(aq) + 2H*(aq) + 2e PbO,(s) + 4H'(aq) + SO (aq) + 2e Ce**(aq) + e MnO, (aq) + 8H*(aq) + 5e Au'" (ag) + Зe Cl,(g) + 2e Cr,0? (aq) + 14H*(aq) + 6e° MnO,(s) + 4H*(aq) + 2e O2(8) + 4H (aq) + 4e Br2(1) + 2e NO, (aq) + 4H*(aq) + 3e 2H9²*(aq) + 2e Hg3" (aq) + 2e Ag*(aq) + e Fe* (aq) + e O,(g) + 2H*(aq) + 2e¯ MnO, (aq) + 2H,0 + 3e¯ → Mn0;(8) + 40H (ag) L(s) + 2e 0,(g) + 2H,0 + 4e Cu²*(aq) + 2e' AgCI(s) + e SO, (aq) + 4H*(aq) + 2e → SO-(g) + 2H20 4 Cu²*(aq) + e Sn** (aq) + 2e 2H*(aq) + 2e Pb* (aд) + 2e Sn2+(aq) + 2e Ni²* (aq) + 2e Со* (ад) + 2е' PbSO,(s) + 2e Cd²* (aq) + 2e Fe2*(aq) + 2e Cr*(aq) + 3e Zn*(aq) + 2e 2H20 + 2e Mn²*(aq) + 2e АР"(ag) + Зе Bе* (аq) + 2е Mg* (aq) + 2е Na*(ag) + e Са* (ад) + 2e Sr* (ag) + 2e Bа** (ад) + 2е' к "ад) + е Li*(aq) + e → 2F (aq) +2.87 A +2.07 Co** (aq) +1.82 → 2H,0 +1.77 PbSO,(s) + 2H,0 +1.70 Ce*(aq) +1.61 Mn2+ (aq) + 4H,0 +1.51 Au(s) +1.50 → 2CI (aq) +1.36 → 2Cr**(aq) + 7H,O Mn²*(aq) + 2H,0 +1.33 +1.23 2H,0 +1.23 → 2Br (aq) +1.07 - NO(g) + 2H,0 +0.96 → Hgž*(aq) → 2Hg(l) +0.92 +0.85 +0,80 Ag(s) → Fe2* (aq) +0.77 → H;O2(aq) +0.68 +0.59 21¯(aq) +0,53 » 40H (aq) + Cu(s) +0.40 +0.34 Ag(s) + CI (aq) +0.22 +0.20 Cu*(aq) • Sn²*(aq) +0.15 +0.13 H(g) > Pb(s) > Sn(s) 0.00 -0.13 -0.14 Ni(s) -0.25 Co(s) -0.28 Pb(s) + So (aq) -0.31 Cd(s) -0.40 · Fe(s) Cr(s) → Zn(s) » H,(g) + 20H¯(aq) -0.44 -0.74 -0.76 -0.83 Mn(s) -1.18 Al(s) -1.66 Be(s) -1.85 Mg(s) Na(s) → Ca(s) -2.37 -2.71 -2,87 Sr(s) -2.89 Ba(s) -2.90 K(s) -2.93 Li(s) -3.05 "For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases. These are the standard-state values. Increasing strength as oxidizing agent Increasing strength as reducing agent
Transcribed Image Text:TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E°(V) F-(g) + 2e O3(g) + 2H*(aq) + 2e¯ → 0,(g) + H2O Со" (aq) + e H,O,(aq) + 2H*(aq) + 2e PbO,(s) + 4H'(aq) + SO (aq) + 2e Ce**(aq) + e MnO, (aq) + 8H*(aq) + 5e Au'" (ag) + Зe Cl,(g) + 2e Cr,0? (aq) + 14H*(aq) + 6e° MnO,(s) + 4H*(aq) + 2e O2(8) + 4H (aq) + 4e Br2(1) + 2e NO, (aq) + 4H*(aq) + 3e 2H9²*(aq) + 2e Hg3" (aq) + 2e Ag*(aq) + e Fe* (aq) + e O,(g) + 2H*(aq) + 2e¯ MnO, (aq) + 2H,0 + 3e¯ → Mn0;(8) + 40H (ag) L(s) + 2e 0,(g) + 2H,0 + 4e Cu²*(aq) + 2e' AgCI(s) + e SO, (aq) + 4H*(aq) + 2e → SO-(g) + 2H20 4 Cu²*(aq) + e Sn** (aq) + 2e 2H*(aq) + 2e Pb* (aд) + 2e Sn2+(aq) + 2e Ni²* (aq) + 2e Со* (ад) + 2е' PbSO,(s) + 2e Cd²* (aq) + 2e Fe2*(aq) + 2e Cr*(aq) + 3e Zn*(aq) + 2e 2H20 + 2e Mn²*(aq) + 2e АР"(ag) + Зе Bе* (аq) + 2е Mg* (aq) + 2е Na*(ag) + e Са* (ад) + 2e Sr* (ag) + 2e Bа** (ад) + 2е' к "ад) + е Li*(aq) + e → 2F (aq) +2.87 A +2.07 Co** (aq) +1.82 → 2H,0 +1.77 PbSO,(s) + 2H,0 +1.70 Ce*(aq) +1.61 Mn2+ (aq) + 4H,0 +1.51 Au(s) +1.50 → 2CI (aq) +1.36 → 2Cr**(aq) + 7H,O Mn²*(aq) + 2H,0 +1.33 +1.23 2H,0 +1.23 → 2Br (aq) +1.07 - NO(g) + 2H,0 +0.96 → Hgž*(aq) → 2Hg(l) +0.92 +0.85 +0,80 Ag(s) → Fe2* (aq) +0.77 → H;O2(aq) +0.68 +0.59 21¯(aq) +0,53 » 40H (aq) + Cu(s) +0.40 +0.34 Ag(s) + CI (aq) +0.22 +0.20 Cu*(aq) • Sn²*(aq) +0.15 +0.13 H(g) > Pb(s) > Sn(s) 0.00 -0.13 -0.14 Ni(s) -0.25 Co(s) -0.28 Pb(s) + So (aq) -0.31 Cd(s) -0.40 · Fe(s) Cr(s) → Zn(s) » H,(g) + 20H¯(aq) -0.44 -0.74 -0.76 -0.83 Mn(s) -1.18 Al(s) -1.66 Be(s) -1.85 Mg(s) Na(s) → Ca(s) -2.37 -2.71 -2,87 Sr(s) -2.89 Ba(s) -2.90 K(s) -2.93 Li(s) -3.05 "For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases. These are the standard-state values. Increasing strength as oxidizing agent Increasing strength as reducing agent
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