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
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...
Related questions
Question
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16f65cf9-d3bb-4ef1-8d11-46be7a9043fa%2Fd3411ba5-8a96-4433-a77d-73ef5502b489%2Fu1luno_processed.png&w=3840&q=75)
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);](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16f65cf9-d3bb-4ef1-8d11-46be7a9043fa%2Fd3411ba5-8a96-4433-a77d-73ef5502b489%2Fcflcti_processed.png&w=3840&q=75)
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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