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1. What should be the reaction at the cathode? a. Fe³+ (aq) + e- → Fe²+ (aq) Ag (aq) + e → Ag(s) b. c. d. Fe²+ (aq) → Fe³+ (aq) + e- Ag(s) Ag*(aq) + e- None of the given. e. 2. What will be the Eᵒcell? a. -0.22 V b. -0.03 V C. +0.36 V d. +1.24 V e. None of the given. 3. What will be the species present in the solution in cathode compartment? a. Fe³+ (aq) & Fe²+ (aq)Ag*(aq) b. Agt(aq) & Fe²+ (aq) c. Fe³+ (aq) d. None of the given. 4. What can serve as the electrode in the anode compartment? a. Pt(s) b. Ag(s) c. Fe(s) d. Fe²+(s) e. None of the given. 5. What is the cell diagram? b. a. Ag(s) | Agt(aq) || Fe³+ (aq), Fe²+ (aq) | Fe(s) Fe(s) | Fe³+ (aq), Fe²+ (aq) || Ag*(aq) | Ag(s) Pt(s) | Fe³+ (aq), Fe²+ (aq) || Ag+(aq) | Ag(s) Ag(s) | Ag+ (aq) || Fe³+ (aq), Fe²+ (aq) | Pt(s) None of the given. c. d. e.

1. What should be the reaction at the cathode? a. Fe³+ (aq) + e- → Fe²+ (aq) Ag (aq) + e → Ag(s) b. c. d. Fe²+ (aq) → Fe³+ (aq) + e- Ag(s) Ag*(aq) + e- None of the given. e. 2. What will be the Eᵒcell? a. -0.22 V b. -0.03 V C. +0.36 V d. +1.24 V e. None of the given. 3. What will be the species present in the solution in cathode compartment? a. Fe³+ (aq) & Fe²+ (aq)Ag*(aq) b. Agt(aq) & Fe²+ (aq) c. Fe³+ (aq) d. None of the given. 4. What can serve as the electrode in the anode compartment? a. Pt(s) b. Ag(s) c. Fe(s) d. Fe²+(s) e. None of the given. 5. What is the cell diagram? b. a. Ag(s) | Agt(aq) || Fe³+ (aq), Fe²+ (aq) | Fe(s) Fe(s) | Fe³+ (aq), Fe²+ (aq) || Ag*(aq) | Ag(s) Pt(s) | Fe³+ (aq), Fe²+ (aq) || Ag+(aq) | Ag(s) Ag(s) | Ag+ (aq) || Fe³+ (aq), Fe²+ (aq) | Pt(s) None of the given. c. d. e.

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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For a galvanic cell based on the following half-reactions:

Fe3+(aq) + e- → Fe2+(aq)
Ag+(aq) + e- → Ag(s)

1. What should be the reaction at the cathode? a. Fe³+ (aq) + e → Fe²+ (aq) b. Ag (aq) + e → Ag(s) c. Fe²+ (aq) → Fe³+ (aq) + e- Ag(s) Ag*(aq) + e- d. e. None of the given. 2. What will be the Eᵒcell? a. -0.22 V b. -0.03 V C. +0.36 V d. +1.24 V e. None of the given. What will be the species present in the solution in cathode compartment? a. Fe³+ (aq) & Fe²+ (aq)Ag*(aq) b. Agt(aq) & Fe²+ (aq) c. Fe³+ (aq) d. None of the given. 4. What can serve as the electrode in the anode compartment? a. Pt(s) b. Ag(s) c. Fe(s) d. Fe²+(s) e. None of the given. 5. What is the cell diagram? b. a. Ag(s) | Ag+ (aq) || Fe³+ (aq), Fe²+ (aq) | Fe(s) Fe(s) | Fe³+ (aq), Fe²+ (aq) || Ag+ (aq) | Ag(s) Pt(s) | Fe³+ (aq), Fe²+ (aq) || Ag+(aq) | Ag(s) Ag(s) | Agt(aq) || Fe³+ (aq), Fe²+ (aq) | Pt(s) None of the given. c. d. e.
Transcribed Image Text:1. What should be the reaction at the cathode? a. Fe³+ (aq) + e → Fe²+ (aq) b. Ag (aq) + e → Ag(s) c. Fe²+ (aq) → Fe³+ (aq) + e- Ag(s) Ag*(aq) + e- d. e. None of the given. 2. What will be the Eᵒcell? a. -0.22 V b. -0.03 V C. +0.36 V d. +1.24 V e. None of the given. What will be the species present in the solution in cathode compartment? a. Fe³+ (aq) & Fe²+ (aq)Ag*(aq) b. Agt(aq) & Fe²+ (aq) c. Fe³+ (aq) d. None of the given. 4. What can serve as the electrode in the anode compartment? a. Pt(s) b. Ag(s) c. Fe(s) d. Fe²+(s) e. None of the given. 5. What is the cell diagram? b. a. Ag(s) | Ag+ (aq) || Fe³+ (aq), Fe²+ (aq) | Fe(s) Fe(s) | Fe³+ (aq), Fe²+ (aq) || Ag+ (aq) | Ag(s) Pt(s) | Fe³+ (aq), Fe²+ (aq) || Ag+(aq) | Ag(s) Ag(s) | Agt(aq) || Fe³+ (aq), Fe²+ (aq) | Pt(s) None of the given. c. d. e.
Increasing strength as oxidizing agent Table of Standard Reduction Potentials Half-Reaction F₂(g) + 2e →→→ 2F¯ (aq) O3(g) + 2H¹ (aq) + 2e¯ → O₂(g) + H₂O Co³+ (aq) + e → Co (aq) H₂O₂(aq) + 2H(aq) + 2e → 2H₂O PbO₂ (s) + 4H+ (aq) + SO²(aq) Ce+ (aq) + e Ce³+ (aq) + 2e¯ →→→ PbSO4(s) + 2H₂O 2+ →Mn²+ (aq) + 4H₂O MnO4 (aq) + 8H+ (aq) + 5e7 Au³+ (aq) + 3e - Au(s) Cl₂(g) + 2e →→→ 2Cl¯¯(aq) 3+ Cr₂O² (aq) + 14H*(aq) + 6e¯ 2Cr³+ (aq) + 7H₂O 2+ MnO₂ (s) + 4H+ (aq) + 2e7 →→Mn²+ (aq) + 2H₂O O₂(g) + 4H+ (aq) + 4e¯ →→→ 2H₂O Br₂() +2e7 →→→→2Br (aq) NO3(aq) + 4H+ (aq) + 3e¯→→→→→ NO(g) + 2H₂O 2Hg²+ (aq) + 2e Hg2+ (aq) Hg2+ (aq) + 2e → 2Hg(1) Ag+ (aq) + e → Ag(s) Fe³+ (aq) + e→→→→→ Fe²+ (aq) O₂(g) + 2H+ (aq) + 2e7 →→→→H₂O₂(aq) MnO4 (aq) + 2H₂O + 3e7 1₂(s) + 2e 21 (aq) O₂(g) + 2H₂O + 4e¯ →→→40H(aq) Cu(s) Cu²+ (aq) + 2e AgCl(s) + e Ag(s) + Cl(aq) SO (aq) + 4H+ (aq) + 2e¯ Cu²+ (aq) + e Cu (aq) Sn4+ (aq) + 2e 2H(aq) + 2e Pb²+ (aq) + 2e- Sn²+ (aq) + 2e Ni²+ (aq) + 2e Co²+ (aq) + 2e PbSO4(s) + 2e Cd²+ (aq) + 2e Fe²+ (aq) + 2e Cr³+ (aq) + 3e Zn²+ (aq) + 2e 2H₂O + 2e Mn²+ (aq) + 2e A1³+ (aq) + 3e¯ Be²+ (aq) + 2e Mg2+ (aq) + 2e Na (aq) + e 2+ Ca²+ (aq) + 2e Sr²+ (aq) + 2e Ba²+ (aq) + 2e K+ (aq) + e → K(s) Li (aq) + e → Li(s) Sn²+ (aq) H₂(g) Pb(s) Sn(s) Ni(s) Co(s) → Pb(s) + SO² (aq) Cd(s) Fe(s) Cr(s) Zn(s) H₂(g) + 2OH(aq) →→ Mn(s) Al(s) Be(s) Mg(s) Na(s) MnO₂ (s) + 40H(aq) SO₂(g) + 2H₂O Ca(s) Sr(s) →Ba(s) E°(V) +2.87 +2.07 +1.82 +1.77 +1.70 +1.61 +1.51 +1.50 +1.36 +1.33 +1.23 +1.23 +1.07 +0.96 +0.92 +0.85 +0.80 +0.77 +0.68 +0.59 +0.53 +0.40 +0.34 +0.22 +0.20 +0.15 +0.13 0.00 -0.13 -0.14 -0.25 -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 -0.83 -1.18 -1.66 -1.85 -2.37 -2.71 -2.87 -2.89 -2.90 -2.93 -3.05 Increasing strength as reducing agent
Transcribed Image Text:Increasing strength as oxidizing agent Table of Standard Reduction Potentials Half-Reaction F₂(g) + 2e →→→ 2F¯ (aq) O3(g) + 2H¹ (aq) + 2e¯ → O₂(g) + H₂O Co³+ (aq) + e → Co (aq) H₂O₂(aq) + 2H(aq) + 2e → 2H₂O PbO₂ (s) + 4H+ (aq) + SO²(aq) Ce+ (aq) + e Ce³+ (aq) + 2e¯ →→→ PbSO4(s) + 2H₂O 2+ →Mn²+ (aq) + 4H₂O MnO4 (aq) + 8H+ (aq) + 5e7 Au³+ (aq) + 3e - Au(s) Cl₂(g) + 2e →→→ 2Cl¯¯(aq) 3+ Cr₂O² (aq) + 14H*(aq) + 6e¯ 2Cr³+ (aq) + 7H₂O 2+ MnO₂ (s) + 4H+ (aq) + 2e7 →→Mn²+ (aq) + 2H₂O O₂(g) + 4H+ (aq) + 4e¯ →→→ 2H₂O Br₂() +2e7 →→→→2Br (aq) NO3(aq) + 4H+ (aq) + 3e¯→→→→→ NO(g) + 2H₂O 2Hg²+ (aq) + 2e Hg2+ (aq) Hg2+ (aq) + 2e → 2Hg(1) Ag+ (aq) + e → Ag(s) Fe³+ (aq) + e→→→→→ Fe²+ (aq) O₂(g) + 2H+ (aq) + 2e7 →→→→H₂O₂(aq) MnO4 (aq) + 2H₂O + 3e7 1₂(s) + 2e 21 (aq) O₂(g) + 2H₂O + 4e¯ →→→40H(aq) Cu(s) Cu²+ (aq) + 2e AgCl(s) + e Ag(s) + Cl(aq) SO (aq) + 4H+ (aq) + 2e¯ Cu²+ (aq) + e Cu (aq) Sn4+ (aq) + 2e 2H(aq) + 2e Pb²+ (aq) + 2e- Sn²+ (aq) + 2e Ni²+ (aq) + 2e Co²+ (aq) + 2e PbSO4(s) + 2e Cd²+ (aq) + 2e Fe²+ (aq) + 2e Cr³+ (aq) + 3e Zn²+ (aq) + 2e 2H₂O + 2e Mn²+ (aq) + 2e A1³+ (aq) + 3e¯ Be²+ (aq) + 2e Mg2+ (aq) + 2e Na (aq) + e 2+ Ca²+ (aq) + 2e Sr²+ (aq) + 2e Ba²+ (aq) + 2e K+ (aq) + e → K(s) Li (aq) + e → Li(s) Sn²+ (aq) H₂(g) Pb(s) Sn(s) Ni(s) Co(s) → Pb(s) + SO² (aq) Cd(s) Fe(s) Cr(s) Zn(s) H₂(g) + 2OH(aq) →→ Mn(s) Al(s) Be(s) Mg(s) Na(s) MnO₂ (s) + 40H(aq) SO₂(g) + 2H₂O Ca(s) Sr(s) →Ba(s) E°(V) +2.87 +2.07 +1.82 +1.77 +1.70 +1.61 +1.51 +1.50 +1.36 +1.33 +1.23 +1.23 +1.07 +0.96 +0.92 +0.85 +0.80 +0.77 +0.68 +0.59 +0.53 +0.40 +0.34 +0.22 +0.20 +0.15 +0.13 0.00 -0.13 -0.14 -0.25 -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 -0.83 -1.18 -1.66 -1.85 -2.37 -2.71 -2.87 -2.89 -2.90 -2.93 -3.05 Increasing strength as reducing agent
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