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1. Based on the standard reduction potentials in Table 2, which of the following metals could provide cathodic protection to iron: Al, Cu, Ni, Zn?

1. Based on the standard reduction potentials in Table 2, which of the following metals could provide cathodic protection to iron: Al, Cu, Ni, Zn?

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please answer #4 type the answer or write it clearly so i can understand please
Half-Reaction E°(V) F(g) + 2e - 2F (aq) O,(g) + 2H*(aq) + 2e Co**(aq) + e H,O,(aq) + 2H *(ag) + 2e 2H,0 PhO2(s) + 4H*(aq) + SO (aq) + 2e PhSO,(s) + 2H2O Ce**(ag) + e Ce (aq) MnO, (aq) + 8H*(aq) 5e Aut +2.87 → 0;(g) + H;O +2.07 Co (aq) +1.82 +1.77 +1.70 +1.61 - Mn* (aq) + 4H,0 +1.51 (aq) + 3e Cl,(g) + 2e 2CI (aq) Cr,0 (aq) + 14H*(aq) + 6e MnO,(s) + 4H (aq) + 2e O,(g) + 4H (aq) + 4e Br;(1) + 2e NO, (aq) + 4H*(aq) + 3e- 2Hg (aq) + 2e Hg3"(aq) + 2e Ag*(aq) + e Fe* (aq) + e O,(g) + 2H*(aq) + 2e MnO, (aq) + 2H,0 + 3e L,(s) + 2e -→ 21 (aq) 0,(g) + 2H,0 + 4e Cu2* (ag) + 2e AgCl(s) + e so (aq) + 4H (aq) + 2e Cu²*(aq) + e Sn** (aq) + 2e 2H*(aq) + 2e- Pb2* (aq) + 2e Sn2*(aq) + 2e Ni²* (aq) + 2e Co*(aq) + 2e PbSO,(s) + 2e Cd* (ag) + 2e Fe*(aq) + 2e Cr* (aq) + 3e Zn*(aq) + 2e 2H,0 + 2e Mn*(ag) + 2e Al*(aq) + 3e Be? (aq) + 2e Mg2*(ag) + 2e Na*(aq) + e Ca* (aq) + 2e Sr* (ag) + 2e Ba*(ag) + 2e Ba(s) K*(aq) + e Li (aq) + e Au(s) +1.50 +1.36 2Cr*(aq) + 7H,0 Mn2 (ag) + 2H,O +1.33 +1.23 2H,0 +1.23 2Br (aq) +1.07 NO(g) + 2H,0 +0.96 Hg" (aq) 2Hg(l) Ag(s) Fe (aq) +0.92 +0.85 +0.80 +0.77 → H,O(aq) MnO,(s) + 40H (aq) +0.68 +0.59 +0.53 40H (aq) → Cu(s) + Ag(s) + Cl (aq) +0.40 +0.34 +0.22 → SO,(g) + 2H,0 +0.20 Cu*(aq) Sn (aq) +0.15 +0.13 H2(g) 0.00 Ph(s) -0.13 → Sn(s) → Ni(s) → Co(s) → Pb(s) + S0 (aq) -0.14 -0.25 -0.28 -0.31 Cd(s) -0.40 → Fe(s) - Cr(s) -0.44 -0.74 Zn(s) -0.76 H2(g) + 20H (aq) - Mn(s) -0.83 -1.18 Al(s) -1.66 Be(s) -1.85 → Mg(s) - 2.37 Na(s) -2.71 → Ca(s) -2.87 Sr(s) -2.89 -2.90 » K(s) → Li(s) -2.93 -3.05
Transcribed Image Text:Half-Reaction E°(V) F(g) + 2e - 2F (aq) O,(g) + 2H*(aq) + 2e Co**(aq) + e H,O,(aq) + 2H *(ag) + 2e 2H,0 PhO2(s) + 4H*(aq) + SO (aq) + 2e PhSO,(s) + 2H2O Ce**(ag) + e Ce (aq) MnO, (aq) + 8H*(aq) 5e Aut +2.87 → 0;(g) + H;O +2.07 Co (aq) +1.82 +1.77 +1.70 +1.61 - Mn* (aq) + 4H,0 +1.51 (aq) + 3e Cl,(g) + 2e 2CI (aq) Cr,0 (aq) + 14H*(aq) + 6e MnO,(s) + 4H (aq) + 2e O,(g) + 4H (aq) + 4e Br;(1) + 2e NO, (aq) + 4H*(aq) + 3e- 2Hg (aq) + 2e Hg3"(aq) + 2e Ag*(aq) + e Fe* (aq) + e O,(g) + 2H*(aq) + 2e MnO, (aq) + 2H,0 + 3e L,(s) + 2e -→ 21 (aq) 0,(g) + 2H,0 + 4e Cu2* (ag) + 2e AgCl(s) + e so (aq) + 4H (aq) + 2e Cu²*(aq) + e Sn** (aq) + 2e 2H*(aq) + 2e- Pb2* (aq) + 2e Sn2*(aq) + 2e Ni²* (aq) + 2e Co*(aq) + 2e PbSO,(s) + 2e Cd* (ag) + 2e Fe*(aq) + 2e Cr* (aq) + 3e Zn*(aq) + 2e 2H,0 + 2e Mn*(ag) + 2e Al*(aq) + 3e Be? (aq) + 2e Mg2*(ag) + 2e Na*(aq) + e Ca* (aq) + 2e Sr* (ag) + 2e Ba*(ag) + 2e Ba(s) K*(aq) + e Li (aq) + e Au(s) +1.50 +1.36 2Cr*(aq) + 7H,0 Mn2 (ag) + 2H,O +1.33 +1.23 2H,0 +1.23 2Br (aq) +1.07 NO(g) + 2H,0 +0.96 Hg" (aq) 2Hg(l) Ag(s) Fe (aq) +0.92 +0.85 +0.80 +0.77 → H,O(aq) MnO,(s) + 40H (aq) +0.68 +0.59 +0.53 40H (aq) → Cu(s) + Ag(s) + Cl (aq) +0.40 +0.34 +0.22 → SO,(g) + 2H,0 +0.20 Cu*(aq) Sn (aq) +0.15 +0.13 H2(g) 0.00 Ph(s) -0.13 → Sn(s) → Ni(s) → Co(s) → Pb(s) + S0 (aq) -0.14 -0.25 -0.28 -0.31 Cd(s) -0.40 → Fe(s) - Cr(s) -0.44 -0.74 Zn(s) -0.76 H2(g) + 20H (aq) - Mn(s) -0.83 -1.18 Al(s) -1.66 Be(s) -1.85 → Mg(s) - 2.37 Na(s) -2.71 → Ca(s) -2.87 Sr(s) -2.89 -2.90 » K(s) → Li(s) -2.93 -3.05
1. Using data in Table 1 (see next page), calculate the standard emf for a cell that employs the following overall cell reaction: 2AI(s) + 31(s) → 2 Al3+ (ag) + 6I° (ag) 2. Using Table 1, rank the following species from the strongest to the weakest reducing agent: I (ag), Fe(s), Al(s). Explain why. 3. Using the standard reduction potentials in Table 2, calculate the equilibrium constant at 25°C for the reaction Br2(1) + 2C1(ag) Cl2(g) + 2 Br(aq) 4. Based on the standard reduction potentials in Table 2, which of the following metals could provide çathodic protection to iron: Al, Cu, Ni, Zn? 5. The electrolysis of CuCI(ag) produces Cu(s) and Cl2(g). What is the minimum external emf needed to drive this electrolysis under standard conditions?
Transcribed Image Text:1. Using data in Table 1 (see next page), calculate the standard emf for a cell that employs the following overall cell reaction: 2AI(s) + 31(s) → 2 Al3+ (ag) + 6I° (ag) 2. Using Table 1, rank the following species from the strongest to the weakest reducing agent: I (ag), Fe(s), Al(s). Explain why. 3. Using the standard reduction potentials in Table 2, calculate the equilibrium constant at 25°C for the reaction Br2(1) + 2C1(ag) Cl2(g) + 2 Br(aq) 4. Based on the standard reduction potentials in Table 2, which of the following metals could provide çathodic protection to iron: Al, Cu, Ni, Zn? 5. The electrolysis of CuCI(ag) produces Cu(s) and Cl2(g). What is the minimum external emf needed to drive this electrolysis under standard conditions?
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