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What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cd(s)|Cd2+(0.25 M) ǁ Cl2(g)| Cl ̶ (0.25M)|Pt(s)

What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cd(s)|Cd2+(0.25 M) ǁ Cl2(g)| Cl ̶ (0.25M)|Pt(s)

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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What is the voltage of the following cell?
Use the Reduction Potential Table found in Chapter 17 notes. Cd(s)|Cd2+(0.25 M) ǁ Cl2(g)| Cl ̶ (0.25M)|Pt(s)

Table 19.1 Standard Reduction Potentials at 25°C* Increasing strength as oxidizing agent Half-Reaction F₂(g) + 2e-→→→2F (aq) O3(g) + 2H(aq) + 2e O₂(g) + H₂O Co³+ (aq) + e _ Co+(aq) H₂O₂(aq) + 2H+ (aq) + 2e →→→→→→ 2H₂O PbO₂ (s) + 4H+(aq) + SO2 (aq) + 2e →→PbSO4(s) + 2H₂O Ce+ (aq) + e-Ce³+ (aq) Mn²+ (aq) + 4H₂O MnO (aq) + 8H (aq) + 5e7 Au³+ (aq) + 3e →→→→→→→ Au(s) Cl₂(g) + 2e →→→→2Cl(aq) Cr₂O2 (aq) + 14H*(aq) + 6e¯ →→→2Cr³+ (aq) + 7H₂O MnO₂(s) + 4H*(aq) + 2e Mn²+ (aq) + 2H₂O O₂(g) + 4H+ (aq) + 4e2H₂O Br₂(l) +2e 2Br (aq) NO3(aq) + 4H(aq) + 3e →→→ NO(g) + 2H₂O 2Hg2+ (aq) + 2e → Hg2+ (aq) Hg2+ (aq) + 2e →→→ 2Hg() Ag (aq) + e → Ag(s) Fe³+ (aq) + e →→→Fe²+ (aq) O₂(g) + 2H+ (aq) + 2e MnO4 (aq) + 2H₂O + 3e¯ 12(s) + 2e21 (aq) O₂(g) + 2H₂O + 4e¯ →→→40H (aq) Cu²+ (aq) + 2e → Cu(s) Cd²+ (aq) + 2e Fe2+ (aq) + 2e7 Cr³+(aq) + 3e Zn²+ (aq) + 2e 2H₂O + 2e Mn²+(aq) + 2e™ Al³+ (aq) + 3e Be2+(aq) + 2e Mg²+(aq) + 2e AgCl(s) + e →→ Ag(s) + Cl¯(aq) SO2 (aq) + 4H+ (aq) + 2e SO₂(g) + 2H₂O Cu²+ (aq) + e Sn4+ (aq) + 2e Cu (aq) -Sn²+(aq) 2H+ (aq) + 2e Pb²+(aq) + 2e¯ Sn²+(aq) + 2e- Ni2+(aq) + 2e Co²+(aq) + 2e PbSO4(s) + 2e Nat(aq) + e Ca²+(aq) + 2e - H₂(g) Pb(s) Sn(s) → Ni(s) → Cd(s) → Fe(s) → Cr(s) → Zn(s) H₂O₂(aq) →Co(s) →Pb(s) + SO2 (aq) MnO₂ (s) + 40H (aq) Al(s) H₂(g) + 2OH(aq) > Mn(s) Be(s) → Mg(s) > Na(s) > Ca(s) Sr2+(aq) + 2e Sr(s) Ba²+(aq) + 2e →→→ Ba(s) K+ (aq) + e -→→→→→K(s) Lit(aq) +e →→→→Li(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 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.
Transcribed Image Text:Table 19.1 Standard Reduction Potentials at 25°C* Increasing strength as oxidizing agent Half-Reaction F₂(g) + 2e-→→→2F (aq) O3(g) + 2H(aq) + 2e O₂(g) + H₂O Co³+ (aq) + e _ Co+(aq) H₂O₂(aq) + 2H+ (aq) + 2e →→→→→→ 2H₂O PbO₂ (s) + 4H+(aq) + SO2 (aq) + 2e →→PbSO4(s) + 2H₂O Ce+ (aq) + e-Ce³+ (aq) Mn²+ (aq) + 4H₂O MnO (aq) + 8H (aq) + 5e7 Au³+ (aq) + 3e →→→→→→→ Au(s) Cl₂(g) + 2e →→→→2Cl(aq) Cr₂O2 (aq) + 14H*(aq) + 6e¯ →→→2Cr³+ (aq) + 7H₂O MnO₂(s) + 4H*(aq) + 2e Mn²+ (aq) + 2H₂O O₂(g) + 4H+ (aq) + 4e2H₂O Br₂(l) +2e 2Br (aq) NO3(aq) + 4H(aq) + 3e →→→ NO(g) + 2H₂O 2Hg2+ (aq) + 2e → Hg2+ (aq) Hg2+ (aq) + 2e →→→ 2Hg() Ag (aq) + e → Ag(s) Fe³+ (aq) + e →→→Fe²+ (aq) O₂(g) + 2H+ (aq) + 2e MnO4 (aq) + 2H₂O + 3e¯ 12(s) + 2e21 (aq) O₂(g) + 2H₂O + 4e¯ →→→40H (aq) Cu²+ (aq) + 2e → Cu(s) Cd²+ (aq) + 2e Fe2+ (aq) + 2e7 Cr³+(aq) + 3e Zn²+ (aq) + 2e 2H₂O + 2e Mn²+(aq) + 2e™ Al³+ (aq) + 3e Be2+(aq) + 2e Mg²+(aq) + 2e AgCl(s) + e →→ Ag(s) + Cl¯(aq) SO2 (aq) + 4H+ (aq) + 2e SO₂(g) + 2H₂O Cu²+ (aq) + e Sn4+ (aq) + 2e Cu (aq) -Sn²+(aq) 2H+ (aq) + 2e Pb²+(aq) + 2e¯ Sn²+(aq) + 2e- Ni2+(aq) + 2e Co²+(aq) + 2e PbSO4(s) + 2e Nat(aq) + e Ca²+(aq) + 2e - H₂(g) Pb(s) Sn(s) → Ni(s) → Cd(s) → Fe(s) → Cr(s) → Zn(s) H₂O₂(aq) →Co(s) →Pb(s) + SO2 (aq) MnO₂ (s) + 40H (aq) Al(s) H₂(g) + 2OH(aq) > Mn(s) Be(s) → Mg(s) > Na(s) > Ca(s) Sr2+(aq) + 2e Sr(s) Ba²+(aq) + 2e →→→ Ba(s) K+ (aq) + e -→→→→→K(s) Lit(aq) +e →→→→Li(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 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.
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