Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M): Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s) e. Which material can serve as the electrode in the anode? f. Which material can serve as the electrode in the cathode? g. Write the cell diagram. h. What will be the E°cell?(use values from the provided SRP table)
Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M): Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s) e. Which material can serve as the electrode in the anode? f. Which material can serve as the electrode in the cathode? g. Write the cell diagram. h. What will be the E°cell?(use values from the provided SRP table)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M):
Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s)
e. Which material can serve as the electrode in the anode?
f. Which material can serve as the electrode in the cathode?
g. Write the cell diagram.
h. What will be the E°cell?(use values from the provided SRP table)
Transcribed Image Text:Half-Reaction
E"(V)
F(g) + 2e - 2F (aq)
O,(g) + 2H (aq) + 2e
Co" (ag) + e Co" (aq)
H;O;(aq) + 2H (aq) + 2e 2H;0
PbO;(s) + 4H (aq) + so (aq) + 2e PbSO,(s) + 2H,0
Cet" (ag) + e Ce"(aq)
Mno, (aq) + 8H' (aq) + Se Mn" (aq) + 4H,0
Au" (ag) + 3e Au(s)
Cl(g) + 2e - 2C1 (aq)
CrO (aq) + 14H' (ag) + be - 2Cr" (aq) + 7H;0
MnO;(s) + 4H' (aq) + 2e Mn" (aq) + 2H,0
O,(g) + 4H*(aq) + 4e 2H;0
Br() + 2e - 2Br (aq)
NO, (aq) + 4H' (aq) + 3e
2Hg" (aq) + 2e – Hg" (ag)
Hg" (aq) + 2e 2Hg()
Ag (aq) + e Ag(s)
Fe" (aq) + e
O;(g) + 2H* (aq) + 2e H;O,(aq)
MnO, (aq) + 2H;0 + 3e -
Iz(s) + 2e- 21 (ag)
O,(g) + 2H,0 + 4e 40H (ag)
Cu" (aq) + 2e Cu(s)
* ABCI(s) + e - Ag(s) + CI (aq)
so, (ag) + 4H'(aq) + 2e SO;(g) + 2H;0
Cu" (ag) + e
Sn* (ag) + 2e Sn" (aq)
2H (aq) + 2e"
Pb"
+2.87
+ 0,(8) + H,0
+2.07
+1.82
+1.77
+1.70
+1.61
+1.51
+1.50
+1.36
+1.33
+1.23
+1.23
+1.07
+ NO(g) + 2H;O
+0.96
+0.92
+0.85
+0.80
+0.77
- Fe* (aq)
+0.68
+ MnO,(s) + 4OH (aq)
+0.59
+0.53
+0.40
+0.34
+0.22
+0.20
Cu" (ag)
+0.15
+0.13
H(g)
0.00
(aq) + 2e - Pb(s)
Sn" (ag) + 2e
Ni* (aq) + 2e Ni(s)
Co" (aq) + 2e Co(s)
PbSO,(s) + 2e - Pb(s) + so (ag)
-0.13
Sn(s)
--0.14
-0.25
-0.28
-0.31
Increasing strength as oxidizing agent
Increasing strength as reducing agent
Transcribed Image Text:Co" (aq) + 2e
PbSO,(s) + 2e
Ca* (aq) + 2e
Fe" (aq) + 2e Fe(s)
C*(aq) + 3e Cr(s)
Zn* (aq) + 2e – Zn(s)
2H,0 + 2e H;(g) + 20H (aq)
Mn" (ag) + 2e
Al" (aq) + 3e Al(s)
Be" (aq) + 2e → Be(s)
Mg" (ag) + 2e - Mg(s)
Na (aq) + e
Ca" (aq) + 2e
Sr"(aq) + 2e Sr(s)
Ba"(aq) + 2e – Ba(s)
K'(aq) + e - K(s)
Li' (aq) + e - Li(s)
+ Co(s)
Pb(s) + So, (ag)
Cd(s)
-0.28
-0.31
-0.40
--0.44
-0.74
-0.76
-0.83
+ Mn(s)
-1.18
-1.66
-1.85
-2.37
+ Na(s)
+ Ca(s)
-2.71
-2.87
-2.89
-2.90
-2.93
-3.05
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