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Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2*(aq) + Ni(s) Hg(1) + Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be than zero.

Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2*(aq) + Ni(s) Hg(1) + Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be than zero.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 110QRT
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Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) + Ag"(aq) + e Ag(s) 0.799 > Hg2"(aq) + 2 e → 2 Hg(1) 0.789 Fe3+ *(aq) + e¯ – Fe2*(aq) 0.771 > 2(s) + 2 e – →21 (aq) 0.535 4- 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 2+ Pb-(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 Cr*(aq) + e→ Cr*(aq) -0.41 Fe2 (aq) + 2 e Fe(s) -0.44 Cr*(aq) + 3 e -→ Cr(s) -0.74 Zn2*(ag) + 2 e Zn(s) -0.763
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction E° (volts) + Ag"(aq) + e Ag(s) 0.799 > Hg2"(aq) + 2 e → 2 Hg(1) 0.789 Fe3+ *(aq) + e¯ – Fe2*(aq) 0.771 > 2(s) + 2 e – →21 (aq) 0.535 4- 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 2+ Pb-(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 Cr*(aq) + e→ Cr*(aq) -0.41 Fe2 (aq) + 2 e Fe(s) -0.44 Cr*(aq) + 3 e -→ Cr(s) -0.74 Zn2*(ag) + 2 e Zn(s) -0.763
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg²*(aq) + Ni(s) Hg(1) + - Ni²*(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be than zero.
Transcribed Image Text:Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg²*(aq) + Ni(s) Hg(1) + - Ni²*(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be than zero.
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