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Using the standard reduction potentials in Table 8-1, place these elements in order of increasing ability to function as reducing agents: a) Cl, b) Fe c) Ag d) Na e) H2

Using the standard reduction potentials in Table 8-1, place these elements in order of increasing ability to function as reducing agents: a) Cl, b) Fe c) Ag d) Na e) H2

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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10. Refer to the attached photo below. Thank you!

Table 8-1 Standard Reduction Potentials in Aqueous Solution at 25°C" Reduction Half Reaction Oxidizing Agents Reducing Agents +2.87 F2(g) + 2 e H,O, (aq) + 2 H;0*(aq) + 2 e PbO,(s) + SO (aq) + 4 H,O* (aq) + 2 e -0.78 V 2F (aq) 4 H,0 (() +1.763 +1.690 PbSO,(s) + 6 H,O(€) Au (aq) + 3 e Au (s) +1.52 MnO, (aq) + 8 H,0 (aq) + 5 e Mn2 (aq) + 12 H,0 (() +1.51 Cr,0; (aq) + 14 H30*(aq) + 6 e 2 Cr*(aq) +21 H,0() +1.36 ones 8-1. Cl,(g) + 2 e +1.358 2 CI (aq) 6 H,0 () 2 Br (aq) rause 0,g) + 4 H,0 (aq) + 4 e +1.229 hich ogen dard Br, (() + 2 e +1.066 NO (aq) + 4 H;0*(aq) + 3 e NO (g) + 6 H,0 () +0.96 - we OCI (aq) + H,0(e) + 2 e CI (aq) + 2 OH (aq) Hg () +0.89 Hg (aq) + 2 e +0.8535 Ag (aq) + e Ag(s) +0.7991 Hg (aq) + 2 e Fe* (aq) + e 2 Hg (e) Fe (aq) +0.7960 V +0.771 (s) + 2 e 21 (aq) +0.535 0,(g) + 2 H,0 (€) + 4 e +4 OH (aq) +0.401 es Cu²t (aq) + 2 e Cu (s) +0.340 e Sn+(aq) + 2 e Sn2+ (aq) +0.15 2 H;0*(aq) + 2 e →H,(g) + 2 H,0 (e) Sn (s) Sn²* (aq) + 2 e 0.1375 Ni2+ (aq) + 2 e Ni (s) 0.25 PbSO, (s) + 2 e Pb(s) +SO (aq) -0.3505 Cd²+(aq) + 2 e Cd (s) -0.403 Fe?+ (aq) + 2 e Fe (s) -0.44 Zn* (aq) + 2 e Zn (s) -0.763 2 H,0 (() + 2 e H2(g) + 2 OH (aq) Al (s) 0.8277 Al+(aq) + 3 e -1.676 Mg+ (aq) + 2 e Mg (s) -2.356 Na (aq) + e Na (s) -2.714 K* (aq) + e K(s) -2.925 Li* (aq) + e Li(s) -3.045 Data from Bard, A. J., Parsons, R., and Jordan, J. Standard Potentials in Aqueous Solution. New York: Marcel Dekker: 1985. International Union of Pure and Applied Chemistry Commission on Electrochemistry and Electroanalytical Chemistry. *In volts (V) versus the standard hydrogen electrode.
Transcribed Image Text:Table 8-1 Standard Reduction Potentials in Aqueous Solution at 25°C" Reduction Half Reaction Oxidizing Agents Reducing Agents +2.87 F2(g) + 2 e H,O, (aq) + 2 H;0*(aq) + 2 e PbO,(s) + SO (aq) + 4 H,O* (aq) + 2 e -0.78 V 2F (aq) 4 H,0 (() +1.763 +1.690 PbSO,(s) + 6 H,O(€) Au (aq) + 3 e Au (s) +1.52 MnO, (aq) + 8 H,0 (aq) + 5 e Mn2 (aq) + 12 H,0 (() +1.51 Cr,0; (aq) + 14 H30*(aq) + 6 e 2 Cr*(aq) +21 H,0() +1.36 ones 8-1. Cl,(g) + 2 e +1.358 2 CI (aq) 6 H,0 () 2 Br (aq) rause 0,g) + 4 H,0 (aq) + 4 e +1.229 hich ogen dard Br, (() + 2 e +1.066 NO (aq) + 4 H;0*(aq) + 3 e NO (g) + 6 H,0 () +0.96 - we OCI (aq) + H,0(e) + 2 e CI (aq) + 2 OH (aq) Hg () +0.89 Hg (aq) + 2 e +0.8535 Ag (aq) + e Ag(s) +0.7991 Hg (aq) + 2 e Fe* (aq) + e 2 Hg (e) Fe (aq) +0.7960 V +0.771 (s) + 2 e 21 (aq) +0.535 0,(g) + 2 H,0 (€) + 4 e +4 OH (aq) +0.401 es Cu²t (aq) + 2 e Cu (s) +0.340 e Sn+(aq) + 2 e Sn2+ (aq) +0.15 2 H;0*(aq) + 2 e →H,(g) + 2 H,0 (e) Sn (s) Sn²* (aq) + 2 e 0.1375 Ni2+ (aq) + 2 e Ni (s) 0.25 PbSO, (s) + 2 e Pb(s) +SO (aq) -0.3505 Cd²+(aq) + 2 e Cd (s) -0.403 Fe?+ (aq) + 2 e Fe (s) -0.44 Zn* (aq) + 2 e Zn (s) -0.763 2 H,0 (() + 2 e H2(g) + 2 OH (aq) Al (s) 0.8277 Al+(aq) + 3 e -1.676 Mg+ (aq) + 2 e Mg (s) -2.356 Na (aq) + e Na (s) -2.714 K* (aq) + e K(s) -2.925 Li* (aq) + e Li(s) -3.045 Data from Bard, A. J., Parsons, R., and Jordan, J. Standard Potentials in Aqueous Solution. New York: Marcel Dekker: 1985. International Union of Pure and Applied Chemistry Commission on Electrochemistry and Electroanalytical Chemistry. *In volts (V) versus the standard hydrogen electrode.
10. Using the standard reduction potentials in Table 8-1, place these elements in order of increasing ability to function as reducing agents: a) Cl2 b) Fe c) Ag d) Na e) H2
Transcribed Image Text:10. Using the standard reduction potentials in Table 8-1, place these elements in order of increasing ability to function as reducing agents: a) Cl2 b) Fe c) Ag d) Na e) H2
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