Use the standard reduction potentials located in the Tables' linked above to calculate the standard free energy change in kJ for the reaction: Fe2+ (aq) + 2Fe2+ (aq) Fe(s) + 2Fe3+ (aq) Answer: kj K for this reaction would be than one.

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 18.96QE
icon
Related questions
Question
100%
Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction:
Fe2+ (aq) + 2Fe2+ (aq) Fe(s) + 2Fe³+ (aq)
Answer:
kj
K for this reaction would be
than one.
Transcribed Image Text:Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Fe2+ (aq) + 2Fe2+ (aq) Fe(s) + 2Fe³+ (aq) Answer: kj K for this reaction would be than one.
Standard Reduction (Electrode) Potentials at 25 °C
Half-Cell Reaction
2 F (aq)
F₂(g) + 2 e
Ce¹(aq) + e
MnO₂ (aq) + 8
Cl₂(g) + 2 e
Cr₂0₂² (aq) + 14 H(aq) + 6 e —> 2 Cr³(aq) + 7 H₂0 (1)
O₂(g) + 4 H* (aq) + 4e-2 H₂0 (1)
Br₂(1) +2 e 2 Br (aq)
NO₂ (aq) + 4 H*(aq) + 3 e° ——» NO(g) + 2 H₂0 (1)
2 Hg2+ (aq) + 2 eHg₂² (aq)
Hg2+ (aq) + 2 eHg(1)
Ag (aq) + e
Ag(s)
Hg₂²*(aq) + 2 e
Ce³+ (aq)
H(aq) + 5 e
2 Cl(aq)
→→→>2 Hg(!)
Fe³+ (aq) + e
1₂ (s) + 2 e →21 (aq)
→→→Fe²+ (aq)
Fe(CN),³(aq) + e > Fe(CN),* (aq)
Cu²+ (aq) + 2 e
Cu(s)
Cu²+ (aq) +
Cu(aq)
S(s) + 2 H¹ (aq) + 2 H₂S(aq)
2 H*(aq) + 2e
Pb²+ (aq) + 2 e
Sn²(aq) + 2 e
Ni²+ (aq) + 2 e
Co²+ (aq) + 2 e
Cd²+ (aq) + 2 e
Cr²³(aq) + e
Fe²+ (aq) + 2 e
Cr³+ (aq) + 3 e
Zn²2(aq) + 2 e
2 H₂O(1) + 2 e
H₂(g)
> Pb(s)
Sn(s)
→→Ni(s)
Co(s)
Cd (s)
Cr²2 (aq)
Mn²+ (aq) + 4H₂O(1)
→→Fe(s)
→→Cr(s)
Zn(s)
> H₂(g) + 2 OH(aq)
Mn²+ (aq) + 2e →→→Mn(s)
Al³+ (aq) + 3 e →→→> Al(s)
Mg2+ (aq) + 2 e
Mg(s)
Na (aq) +eNa(s)
K(aq) + e →→→K(s)
Li (aq) +eLi(s)
Eº (volts)
2.87
1.61
1.51
1.36
1.33
1.229
1.08
0.96
0.920
0.855
0.799
0.789
0.771
0.535
0.48
0.337
0.153
0.14
0.0000
-0.126
-0.14
-0.25
-0.28
-0.403
-0.41
-0.44
-0.74
-0.763
-0.83
-1.18
-1.66
-2.37
-2.714
-2.925
-3.045
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction 2 F (aq) F₂(g) + 2 e Ce¹(aq) + e MnO₂ (aq) + 8 Cl₂(g) + 2 e Cr₂0₂² (aq) + 14 H(aq) + 6 e —> 2 Cr³(aq) + 7 H₂0 (1) O₂(g) + 4 H* (aq) + 4e-2 H₂0 (1) Br₂(1) +2 e 2 Br (aq) NO₂ (aq) + 4 H*(aq) + 3 e° ——» NO(g) + 2 H₂0 (1) 2 Hg2+ (aq) + 2 eHg₂² (aq) Hg2+ (aq) + 2 eHg(1) Ag (aq) + e Ag(s) Hg₂²*(aq) + 2 e Ce³+ (aq) H(aq) + 5 e 2 Cl(aq) →→→>2 Hg(!) Fe³+ (aq) + e 1₂ (s) + 2 e →21 (aq) →→→Fe²+ (aq) Fe(CN),³(aq) + e > Fe(CN),* (aq) Cu²+ (aq) + 2 e Cu(s) Cu²+ (aq) + Cu(aq) S(s) + 2 H¹ (aq) + 2 H₂S(aq) 2 H*(aq) + 2e Pb²+ (aq) + 2 e Sn²(aq) + 2 e Ni²+ (aq) + 2 e Co²+ (aq) + 2 e Cd²+ (aq) + 2 e Cr²³(aq) + e Fe²+ (aq) + 2 e Cr³+ (aq) + 3 e Zn²2(aq) + 2 e 2 H₂O(1) + 2 e H₂(g) > Pb(s) Sn(s) →→Ni(s) Co(s) Cd (s) Cr²2 (aq) Mn²+ (aq) + 4H₂O(1) →→Fe(s) →→Cr(s) Zn(s) > H₂(g) + 2 OH(aq) Mn²+ (aq) + 2e →→→Mn(s) Al³+ (aq) + 3 e →→→> Al(s) Mg2+ (aq) + 2 e Mg(s) Na (aq) +eNa(s) K(aq) + e →→→K(s) Li (aq) +eLi(s) Eº (volts) 2.87 1.61 1.51 1.36 1.33 1.229 1.08 0.96 0.920 0.855 0.799 0.789 0.771 0.535 0.48 0.337 0.153 0.14 0.0000 -0.126 -0.14 -0.25 -0.28 -0.403 -0.41 -0.44 -0.74 -0.763 -0.83 -1.18 -1.66 -2.37 -2.714 -2.925 -3.045
Expert Solution
steps

Step by step

Solved in 3 steps with 3 images

Blurred answer
Knowledge Booster
Electrochemical Cells
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax