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Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);

Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.45QE: Use the data from the table of standard reduction potentials in Appendix H to calculate the standard...
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Chem 1B Chapter-17 Tutorial Worksheet Reduction Potentials of selected substances: PbO2 + HSO, + 3H* + 2e → PBSO, + 2H2O; E = 1.68 V Mno, + 8H* + Se → Mn* + 2H20; E = 1.51 V %3D Au" + 3e → Au; E = 1.50 V Cl2 E = 1.36 V + 2e → 2Cr ; Cr:0 + 14H + 6e → 2Cr* + 7H;O; E - 1,23 V %3D MnO2 + 4H" + 2e → Mn + 2H2O; O, + 4H' + 4e → 2H2O; = 1.23 V E = 1.23 V %3D Brz + 2e → 2Br ; E- 1.09 V NO, + 4H* + 3e → NO + 2H,O; E = 0.96 V E - 0.92 V 2Hg* + 2e -→ Hg.* ; CIO + H;O + 2e → CI + 20H; %3D E = 0.89 V Hg* + 2e - Hg; E = 0.85 V Ag + e Ag; E = 0.80 V E - 0.80 V Hg" + 2e → 2Hg; Fe" + e → Fe"; E - 0.77 V E = 0.76 V %3D Nis + 2e Ni + S; I + 2e 21; E - 0.54 V %3D Cu* + 2e Cu; E = 0.34 V %3D Hg:Cl; + 2e → 2Hg + 2CT; E = 0.28 V %3D Pb+ + 2e Pb; E= -0,13 V %3D Ni' + 2e Ni; E = -0.26 V PBSO4 + H' + 2e → Pb + HSO4; E - -0,36 V %3D Fe" + 2e -→ Fe; E- -0.45 V Ni(NH:),* + 2e → Ni + 6NH3; = -0.50 V E = -0.70 V HgS + 2e -→ Hg + s?; %3D = -0.74 V E- -0.76 V E - -0.95 V Cr" + 3e - Cr; Zn + 2e Zn; PbS + 2e → Pb + S?; Zn(NH:),* + 2e → Zn + 4NH;; Zn(OH)? + 2e → Zn + 4 OH; Zn(OH)2 + 2e → Zn + 2 OH; '= -1.02 V E = -1.20 V E - -1,24 V Zns + 2e -→ Zn + S; E - -1.40 V Al* + 3e - Al; E - -1.66 V Na + e Na; E = -2.71 V K* + e → K; E = -2.93 V Li" + e → Li; E - -3.04 V
Transcribed Image Text:Chem 1B Chapter-17 Tutorial Worksheet Reduction Potentials of selected substances: PbO2 + HSO, + 3H* + 2e → PBSO, + 2H2O; E = 1.68 V Mno, + 8H* + Se → Mn* + 2H20; E = 1.51 V %3D Au" + 3e → Au; E = 1.50 V Cl2 E = 1.36 V + 2e → 2Cr ; Cr:0 + 14H + 6e → 2Cr* + 7H;O; E - 1,23 V %3D MnO2 + 4H" + 2e → Mn + 2H2O; O, + 4H' + 4e → 2H2O; = 1.23 V E = 1.23 V %3D Brz + 2e → 2Br ; E- 1.09 V NO, + 4H* + 3e → NO + 2H,O; E = 0.96 V E - 0.92 V 2Hg* + 2e -→ Hg.* ; CIO + H;O + 2e → CI + 20H; %3D E = 0.89 V Hg* + 2e - Hg; E = 0.85 V Ag + e Ag; E = 0.80 V E - 0.80 V Hg" + 2e → 2Hg; Fe" + e → Fe"; E - 0.77 V E = 0.76 V %3D Nis + 2e Ni + S; I + 2e 21; E - 0.54 V %3D Cu* + 2e Cu; E = 0.34 V %3D Hg:Cl; + 2e → 2Hg + 2CT; E = 0.28 V %3D Pb+ + 2e Pb; E= -0,13 V %3D Ni' + 2e Ni; E = -0.26 V PBSO4 + H' + 2e → Pb + HSO4; E - -0,36 V %3D Fe" + 2e -→ Fe; E- -0.45 V Ni(NH:),* + 2e → Ni + 6NH3; = -0.50 V E = -0.70 V HgS + 2e -→ Hg + s?; %3D = -0.74 V E- -0.76 V E - -0.95 V Cr" + 3e - Cr; Zn + 2e Zn; PbS + 2e → Pb + S?; Zn(NH:),* + 2e → Zn + 4NH;; Zn(OH)? + 2e → Zn + 4 OH; Zn(OH)2 + 2e → Zn + 2 OH; '= -1.02 V E = -1.20 V E - -1,24 V Zns + 2e -→ Zn + S; E - -1.40 V Al* + 3e - Al; E - -1.66 V Na + e Na; E = -2.71 V K* + e → K; E = -2.93 V Li" + e → Li; E - -3.04 V
Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);
Transcribed Image Text:Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);
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