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Using the table of standard electrode potentials, decide which of the following statements is completely true.   a Cl2 can oxidize Cd, and Al3+ can reduce Cu2+. b Cd2+ can oxidize Cu, and Cd2+ can reduce Cl2. c Cu2+ can oxidize Cd, and Cd can reduce Al3+.

Using the table of standard electrode potentials, decide which of the following statements is completely true.   a Cl2 can oxidize Cd, and Al3+ can reduce Cu2+. b Cd2+ can oxidize Cu, and Cd2+ can reduce Cl2. c Cu2+ can oxidize Cd, and Cd can reduce Al3+.

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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Using the table of standard electrode potentials, decide which of the following statements is completely true.



 

a
Cl2 can oxidize Cd, and Al3+ can reduce Cu2+.

b
Cd2+ can oxidize Cu, and Cd2+ can reduce Cl2.

c
Cu2+ can oxidize Cd, and Cd can reduce Al3+.
TABLE 17.1 Standard Reduction Potentials at 25 °C Reduction Half-Reaction E (V) Flg) + 2e H,02laq) + 2H*(aq) + 2 e Mno ,laq) + 8 H*(aq) + 5e Mn"(aq) + 4H,0(1) Clalg) + 2e Cr,0, laq) + 14 H*(aq) + 6e 2Cr*(aq) + 7 H,0(1) Ozlg) + 4H*(aq) + 4e Brzlaq) + 2e Ag *(aq) + e Fe"(aq) + e Weaker Stronger oxidizing agent 2F(aq) 2.87 1.78 reducing 1.51 agent 2 Cr (aq) 1.36 1.33 2H,0(1) 2 Br (aq) - Ag(s) + Fe* (aq) H,0, (aq) 1.23 1.09 0.80 0.77 Olg) + 2H*(aq) + 2e" ls) + 2e O,(g) + 2H,0() + 4e Cu "(aq) + 2e Sn*(aq) + 2e 0.70 21(aq) 0.54 4 OH (aq) + Cu( s) → Sn*"(aq) 0.40 0.34 0.15 2H"(aq) + 2e Halg) Pb(aq) + 2e Ni *taq) + 2e Cd*(aq) + 2 e Fe"(aq) + 2e Zn"(aq) + 2 e Pb(s) -0.13 + Ni( s) - 0.26 Cd(s) -0.40 + Fe(s) Zn(s) - Hl9) + 2 OH" (aq) - Al( s) Mg(s) → Na( s) → Li(s) - 0.45 - 0.76 2 H,0() + 2e AI"laq) + 3e Mg"(aq) + 2 e - 0.83 - 1.66 - 2.37 - 2.71 Weaker oxidizing agent Na "(aq) + e Litaq) + e Stronger reducing agent - 3.04 Table 17-1 Chemistry, S/e 0 2008 Pearson Prentice Hall, Inc.
Transcribed Image Text:TABLE 17.1 Standard Reduction Potentials at 25 °C Reduction Half-Reaction E (V) Flg) + 2e H,02laq) + 2H*(aq) + 2 e Mno ,laq) + 8 H*(aq) + 5e Mn"(aq) + 4H,0(1) Clalg) + 2e Cr,0, laq) + 14 H*(aq) + 6e 2Cr*(aq) + 7 H,0(1) Ozlg) + 4H*(aq) + 4e Brzlaq) + 2e Ag *(aq) + e Fe"(aq) + e Weaker Stronger oxidizing agent 2F(aq) 2.87 1.78 reducing 1.51 agent 2 Cr (aq) 1.36 1.33 2H,0(1) 2 Br (aq) - Ag(s) + Fe* (aq) H,0, (aq) 1.23 1.09 0.80 0.77 Olg) + 2H*(aq) + 2e" ls) + 2e O,(g) + 2H,0() + 4e Cu "(aq) + 2e Sn*(aq) + 2e 0.70 21(aq) 0.54 4 OH (aq) + Cu( s) → Sn*"(aq) 0.40 0.34 0.15 2H"(aq) + 2e Halg) Pb(aq) + 2e Ni *taq) + 2e Cd*(aq) + 2 e Fe"(aq) + 2e Zn"(aq) + 2 e Pb(s) -0.13 + Ni( s) - 0.26 Cd(s) -0.40 + Fe(s) Zn(s) - Hl9) + 2 OH" (aq) - Al( s) Mg(s) → Na( s) → Li(s) - 0.45 - 0.76 2 H,0() + 2e AI"laq) + 3e Mg"(aq) + 2 e - 0.83 - 1.66 - 2.37 - 2.71 Weaker oxidizing agent Na "(aq) + e Litaq) + e Stronger reducing agent - 3.04 Table 17-1 Chemistry, S/e 0 2008 Pearson Prentice Hall, Inc.
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