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Zn and Zn 2+; Cu and Cu 2+ Anode half reaction Cathode half reaction  E° value of the cell (use chart) do the values differ and why?  2. Cu and Cu 2+; Ni and Ni 2+  Anode half reaction Cathode half reaction  which metal strip is bigger and which is smaller?  3. Pb and Pb 2+; Fe and Fe 2+  Anode half reaction Cathode half reaction  which metal strip is bigger and which is smaller?  4. Zn and Zn 2+; Ni and Ni 2+ Anode half reaction Cathode half reaction  which metal strip is bigger and which is smaller?

Zn and Zn 2+; Cu and Cu 2+ Anode half reaction Cathode half reaction  E° value of the cell (use chart) do the values differ and why?  2. Cu and Cu 2+; Ni and Ni 2+  Anode half reaction Cathode half reaction  which metal strip is bigger and which is smaller?  3. Pb and Pb 2+; Fe and Fe 2+  Anode half reaction Cathode half reaction  which metal strip is bigger and which is smaller?  4. Zn and Zn 2+; Ni and Ni 2+ Anode half reaction Cathode half reaction  which metal strip is bigger and which is smaller?

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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1. Zn and Zn 2+; Cu and Cu 2+

Anode half reaction

Cathode half reaction 

E° value of the cell (use chart)

do the values differ and why? 

2. Cu and Cu 2+; Ni and Ni 2+ 

Anode half reaction

Cathode half reaction 

which metal strip is bigger and which is smaller? 

3. Pb and Pb 2+; Fe and Fe 2+ 

Anode half reaction

Cathode half reaction 

which metal strip is bigger and which is smaller? 

4. Zn and Zn 2+; Ni and Ni 2+

Anode half reaction

Cathode half reaction 

which metal strip is bigger and which is smaller? 

TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction Stronger oxidizing agent F₂(g) + 2 e H₂O₂(aq) + 2 H(aq) + 2 e PbO₂ (s) + 4 H(aq) + SO42-(aq) + 2 e™ MnO4 (aq) + 4 H*(aq) + 3 e MnO4 (aq) + 8 H*(aq) + 5 e Au³+ (aq) + 3 e™ PbO₂ (s) + 4 H*(aq) + 2 e Cl₂(g) + 2 e Cr₂0,2 (aq) + 14 H*(aq) + 6 e O₂(g) + 4 H*(aq) + 4 e MnO₂ (s) + 4 H*(aq) + 2 e 10₂ (aq) + 6 H(aq) + 5 e Br₂(l) + 2 e VO₂ (aq) + 2 H+ (aq) + e NO3(aq) + 4 H*(aq) + 3 e CIO₂(g) + e Ag (aq) + e Fe³+ (aq) + e O₂(g) + 2 H(aq) + 2 e MnO4 (aq) + e 12(s) + 2 e Cu (aq) + e O₂(g) + 2 H₂O(l) + 4 e Cu²+ (aq) + 2 e SO2 (aq) + 4 H (aq) + 2 e Cu2+ (aq) + e Sn+ (aq) + 2 e 2 H*(aq) + 2 e Fe³+ (aq) + 3 e Pb2+ (aq) + 2 e Sn²+ (aq) + 2 e Ni2+ (aq) + 2 e Cd²+ (aq) + 2 e™ Fe²+ (aq) + 2 e Cr³+ (aq) + e Cr³+ (aq) + 3 e Zn²+ (aq) + 2 e 2 H₂O(l) + 2 e Mn²+ (aq) + 2 e™ Al³+ (aq) + 3 e Mg2+ (aq) + 2 e Na (aq) + e Ca²+ (aq) + 2 e™ Ba2+ (aq) + 2 e™ K+ (aq) + e 2 F (aq) 2 H₂O(l) PbSO4(s) + 2 H₂O(l) →→→→MnO₂ (s) + 2 H₂O(l) →→Mn²+ (aq) + 4H₂O(l) - - →→→ Au(s) → Pb2+ (aq) + 2 H₂O(l) - 2 Cl(aq) 2 Cr³+ (aq) + 7 H₂O(l) 2 H₂O(l) Mn²+ (aq) + 2 H₂O(1) • }l2(aq) + 3 H,O() 2 Br (aq) - VO²+ (aq) + H₂O(l) - →→→ NO(g) + 2 H₂O(1) CIO₂ (aq) →→→ Ag(s) →→→ Fe²+ (aq) H,O,(aq) →→→MnO₂² (aq) -21 (aq) Cu(s) 4 OH(aq) →→→ Cu(s) → H₂SO3(aq) + H₂O(l) →→→ Cut (aq) Sn²+ (aq) H₂(g) Fe(s) →→→→ Pb(s) →→→→Sn(s) - Ni(s) - Cd(s) →→→→Fe(s) Cr²+ (aq) - Cr(s) →→→ Zn(s) H₂(g) + 2 OH(aq) →→→→Mn(s) Al(s) Mg(s) Na(s) - Ca(s) →→→→→Ba(s) K(s) E°(V) 2.87 1.78 1.69 1.68 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.96 0.95 0.80 0.77 0.70 0.56 0.54 0.52 0.40 0.34 0.20 0.16 0.15 0 -0.036 -0.13 -0.14 -0.23 -0.40 -0.45 -0.50 -0.73 -0.76 -0.83 -1.18 -1.66 -2.37 -2.71 -2.76 -2.90 -2.92 1 | | Weaker reducing agent
Transcribed Image Text:TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction Stronger oxidizing agent F₂(g) + 2 e H₂O₂(aq) + 2 H(aq) + 2 e PbO₂ (s) + 4 H(aq) + SO42-(aq) + 2 e™ MnO4 (aq) + 4 H*(aq) + 3 e MnO4 (aq) + 8 H*(aq) + 5 e Au³+ (aq) + 3 e™ PbO₂ (s) + 4 H*(aq) + 2 e Cl₂(g) + 2 e Cr₂0,2 (aq) + 14 H*(aq) + 6 e O₂(g) + 4 H*(aq) + 4 e MnO₂ (s) + 4 H*(aq) + 2 e 10₂ (aq) + 6 H(aq) + 5 e Br₂(l) + 2 e VO₂ (aq) + 2 H+ (aq) + e NO3(aq) + 4 H*(aq) + 3 e CIO₂(g) + e Ag (aq) + e Fe³+ (aq) + e O₂(g) + 2 H(aq) + 2 e MnO4 (aq) + e 12(s) + 2 e Cu (aq) + e O₂(g) + 2 H₂O(l) + 4 e Cu²+ (aq) + 2 e SO2 (aq) + 4 H (aq) + 2 e Cu2+ (aq) + e Sn+ (aq) + 2 e 2 H*(aq) + 2 e Fe³+ (aq) + 3 e Pb2+ (aq) + 2 e Sn²+ (aq) + 2 e Ni2+ (aq) + 2 e Cd²+ (aq) + 2 e™ Fe²+ (aq) + 2 e Cr³+ (aq) + e Cr³+ (aq) + 3 e Zn²+ (aq) + 2 e 2 H₂O(l) + 2 e Mn²+ (aq) + 2 e™ Al³+ (aq) + 3 e Mg2+ (aq) + 2 e Na (aq) + e Ca²+ (aq) + 2 e™ Ba2+ (aq) + 2 e™ K+ (aq) + e 2 F (aq) 2 H₂O(l) PbSO4(s) + 2 H₂O(l) →→→→MnO₂ (s) + 2 H₂O(l) →→Mn²+ (aq) + 4H₂O(l) - - →→→ Au(s) → Pb2+ (aq) + 2 H₂O(l) - 2 Cl(aq) 2 Cr³+ (aq) + 7 H₂O(l) 2 H₂O(l) Mn²+ (aq) + 2 H₂O(1) • }l2(aq) + 3 H,O() 2 Br (aq) - VO²+ (aq) + H₂O(l) - →→→ NO(g) + 2 H₂O(1) CIO₂ (aq) →→→ Ag(s) →→→ Fe²+ (aq) H,O,(aq) →→→MnO₂² (aq) -21 (aq) Cu(s) 4 OH(aq) →→→ Cu(s) → H₂SO3(aq) + H₂O(l) →→→ Cut (aq) Sn²+ (aq) H₂(g) Fe(s) →→→→ Pb(s) →→→→Sn(s) - Ni(s) - Cd(s) →→→→Fe(s) Cr²+ (aq) - Cr(s) →→→ Zn(s) H₂(g) + 2 OH(aq) →→→→Mn(s) Al(s) Mg(s) Na(s) - Ca(s) →→→→→Ba(s) K(s) E°(V) 2.87 1.78 1.69 1.68 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.96 0.95 0.80 0.77 0.70 0.56 0.54 0.52 0.40 0.34 0.20 0.16 0.15 0 -0.036 -0.13 -0.14 -0.23 -0.40 -0.45 -0.50 -0.73 -0.76 -0.83 -1.18 -1.66 -2.37 -2.71 -2.76 -2.90 -2.92 1 | | Weaker reducing agent
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