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Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 3+ (a) Ga(s) | Ga°* (aq) || Ag" (aq) | Ag(s) 3+ 2+ (b) Zn(s) | Zn* (aq) || Ga™ (aq) | Ga(s) 2+ (c) Zn(s), ZnS(s) | s´ (aq) || Sn^™ (aq) | Sn(s)

Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 3+ (a) Ga(s) | Ga°* (aq) || Ag" (aq) | Ag(s) 3+ 2+ (b) Zn(s) | Zn* (aq) || Ga™ (aq) | Ga(s) 2+ (c) Zn(s), ZnS(s) | s´ (aq) || Sn^™ (aq) | Sn(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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Standard Reduction (Electrode) Potentials at 25 °C Standard Reduction (Electrode) Potentials at 25 °C Half-ell Reaction E (volts) Half-Cell Reaction (volts) Cr"(aq) + 3 e Cr[s) Za"(aq) + 2 e-Zn[s) -0.74 F2(8) + 2 e2 F'(aq) 2.87 -0.763 Ce* (aq) + e' Ce³*(aq) Mno, (aq) + 8 H"(aq) + 5 e Mn²"(aq) + 4 H,0(1) 1.61 2 H,0() + 2 e-Hz(R) + 2 OH (aq) -0.83 1.51 Mn2"(aq) + 2 e- Mn(s) -1.18 Cl2(8) + 2 e 2 cI(aq) 1.36 A"(aq) + 3 e→Al(s) -1.66 Cr20, (aq) + 14 H'(aq) + 6 e' →2 Cr*"(aq) + 7 H20(1) 1.33 Mg2"(aq) + 2 e- Mg(s) -2.37 02(8) + 4 H"(aq) + 4 e2 H20(1) 1.229 Na"(aq) + e Na(s) -2.714 Brz(1) + 2 e 2 Br'(aq) K"(aq) +e K(s) -2.925 1.08 NO, (aq) + 4 H"(aq) + 3 e NO(g) + 2 H,0) Li (aq) + eLi(s) -3.045 0.96 2 Hg2 (aq) + 2 e - Hg,"(aq) 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag"(aq) + e Ag(s) 0.799 Hg,"(aq) + 2 e–2 Hg() 0.789 Fe"(aq) + e Fe²"(aq) 0.771 12(8) + 2 e2 I(aq) 0.535 Fe(CN), (aq) + e' Fe(CN),*(aq) 0.48 Cu2 (aq) + 2 e →Cu(s) 0.337 Cu"(aq) + e Cu"(aq) 0.153 S(s) + 2 H"(aq) + 2 e H,S(aq) 0.14 2 H"(aq) + 2 e- H2(8) 0.0000 Ph (aq) + 2 e' Ph(s) -0.126 Sn2*(aq) + 2 e- Sn(s) -0.14 Ni"(aq) + 2 e NI(s) -0.25 Co2 (aq) + 2 e- Co(s) -0.28 Ca*(aq) + 2 e-Cd(s) -0.403 Cr"(aq) + e Cr²*(aq) -0.41 Fe"(aq) + 2 e Fe(s) -0.44
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Standard Reduction (Electrode) Potentials at 25 °C Half-ell Reaction E (volts) Half-Cell Reaction (volts) Cr"(aq) + 3 e Cr[s) Za"(aq) + 2 e-Zn[s) -0.74 F2(8) + 2 e2 F'(aq) 2.87 -0.763 Ce* (aq) + e' Ce³*(aq) Mno, (aq) + 8 H"(aq) + 5 e Mn²"(aq) + 4 H,0(1) 1.61 2 H,0() + 2 e-Hz(R) + 2 OH (aq) -0.83 1.51 Mn2"(aq) + 2 e- Mn(s) -1.18 Cl2(8) + 2 e 2 cI(aq) 1.36 A"(aq) + 3 e→Al(s) -1.66 Cr20, (aq) + 14 H'(aq) + 6 e' →2 Cr*"(aq) + 7 H20(1) 1.33 Mg2"(aq) + 2 e- Mg(s) -2.37 02(8) + 4 H"(aq) + 4 e2 H20(1) 1.229 Na"(aq) + e Na(s) -2.714 Brz(1) + 2 e 2 Br'(aq) K"(aq) +e K(s) -2.925 1.08 NO, (aq) + 4 H"(aq) + 3 e NO(g) + 2 H,0) Li (aq) + eLi(s) -3.045 0.96 2 Hg2 (aq) + 2 e - Hg,"(aq) 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag"(aq) + e Ag(s) 0.799 Hg,"(aq) + 2 e–2 Hg() 0.789 Fe"(aq) + e Fe²"(aq) 0.771 12(8) + 2 e2 I(aq) 0.535 Fe(CN), (aq) + e' Fe(CN),*(aq) 0.48 Cu2 (aq) + 2 e →Cu(s) 0.337 Cu"(aq) + e Cu"(aq) 0.153 S(s) + 2 H"(aq) + 2 e H,S(aq) 0.14 2 H"(aq) + 2 e- H2(8) 0.0000 Ph (aq) + 2 e' Ph(s) -0.126 Sn2*(aq) + 2 e- Sn(s) -0.14 Ni"(aq) + 2 e NI(s) -0.25 Co2 (aq) + 2 e- Co(s) -0.28 Ca*(aq) + 2 e-Cd(s) -0.403 Cr"(aq) + e Cr²*(aq) -0.41 Fe"(aq) + 2 e Fe(s) -0.44
Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 3+ (a) Ga(s) | Ga" (aq) || Ag" (aq) | Ag(s) 2+ 3+ (b) Zn(s) | Zn (ag) || Ga" (ag) | Ga(8) 2+ (c) Zn(s), ZnS(s) | S´ (ag) || Snª™ (ag) | Sn(s)
Transcribed Image Text:Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 3+ (a) Ga(s) | Ga" (aq) || Ag" (aq) | Ag(s) 2+ 3+ (b) Zn(s) | Zn (ag) || Ga" (ag) | Ga(8) 2+ (c) Zn(s), ZnS(s) | S´ (ag) || Snª™ (ag) | Sn(s)
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