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Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) Fe(CN)6 (aq) + e. Fe(CN),*(aq) 0.48 Cu2 (aq) + 2 e Cu(s) 0.337 Cu2*(aq) + e¯ – Cu*(aq) 0.153 S(s) +2 H"(aq) + 2 e → H2S(aq) 0.14 2 H (aq) + 2 e –→H2(g) 0.0000 Pb2 (aq) + 2 e → Pb(s) -0.126 Sn2+(ag) + 2 e → Sn(s) -0.14

Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) Fe(CN)6 (aq) + e. Fe(CN),*(aq) 0.48 Cu2 (aq) + 2 e Cu(s) 0.337 Cu2*(aq) + e¯ – Cu*(aq) 0.153 S(s) +2 H"(aq) + 2 e → H2S(aq) 0.14 2 H (aq) + 2 e –→H2(g) 0.0000 Pb2 (aq) + 2 e → Pb(s) -0.126 Sn2+(ag) + 2 e → Sn(s) -0.14

Chemistry
Chemistry
9th Edition
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Steven S. Zumdahl
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 150CP: Given the following two standard reduction potentials, solve for the standard reduction potential of...
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Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) Fe(CN)6 (aq) + e→ → Fe(CN),*(aq) 0.48 2+ Cu"(aq) + 2 e →Cu(s) 0.337 Cu2"(aq) + e → Cu*(aq) 0.153 S(s) + 2 H"(aq)+2 e → H2S(aq) 0.14 2 H (aq) + 2 e –→H2(g) 0.0000 Pb2*(aq) + 2 e → Pb(s) -0.126 Sn2*(aq) + 2 e → Sn(s) -0.14 Ni2 (aq) + 2 e - Ni(s) -0.25 Co2*(aq) + 2 e –→ Co(s) -0.28 Cd2*(aq) + 2 e → Cd(s) -0.403 Cr3*(aq) + e Cr*(aq) -0.41 Fe2 (aq) + 2 e –→ Fe(s) -0.44 3+ (aq)+3 e → Cr(s) -0.74 Zn2*(aq) + 2 e → Zn(s) -0.763 2 H20(1) + 2 e → H2(g) + 2 OH (aq) -0.83 Mn2"(aq) + 2 e → Mn(s) -1.18 Al³* (aq) + 3 e–→ Al(s) -1.66 2+ Mg"(aq) + 2 e → Mg(s) -2.37
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) Fe(CN)6 (aq) + e→ → Fe(CN),*(aq) 0.48 2+ Cu"(aq) + 2 e →Cu(s) 0.337 Cu2"(aq) + e → Cu*(aq) 0.153 S(s) + 2 H"(aq)+2 e → H2S(aq) 0.14 2 H (aq) + 2 e –→H2(g) 0.0000 Pb2*(aq) + 2 e → Pb(s) -0.126 Sn2*(aq) + 2 e → Sn(s) -0.14 Ni2 (aq) + 2 e - Ni(s) -0.25 Co2*(aq) + 2 e –→ Co(s) -0.28 Cd2*(aq) + 2 e → Cd(s) -0.403 Cr3*(aq) + e Cr*(aq) -0.41 Fe2 (aq) + 2 e –→ Fe(s) -0.44 3+ (aq)+3 e → Cr(s) -0.74 Zn2*(aq) + 2 e → Zn(s) -0.763 2 H20(1) + 2 e → H2(g) + 2 OH (aq) -0.83 Mn2"(aq) + 2 e → Mn(s) -1.18 Al³* (aq) + 3 e–→ Al(s) -1.66 2+ Mg"(aq) + 2 e → Mg(s) -2.37
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Cu?*(aq) + Fe(s) 2Cu*(aq) + Fe²*(aq) Answer: 114 kJ K for this reaction would be greater than one.
Transcribed Image Text:Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Cu?*(aq) + Fe(s) 2Cu*(aq) + Fe²*(aq) Answer: 114 kJ K for this reaction would be greater than one.
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