Use the data from the redox table (appendix L in the text) to calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given. 1.) AgCl (s) <=> Ag+ (aq) + Cl- (aq)
Use the data from the redox table (appendix L in the text) to calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given. 1.) AgCl (s) <=> Ag+ (aq) + Cl- (aq)
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use the data from the redox table (appendix L in the text) to calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given.
1.) AgCl (s) <=> Ag+ (aq) + Cl- (aq)
![TABLE 18.1 Standard Reduction Potentials in Water at 25°C
Potential (V)
Reduction Half-Reaction
F2(g) + 2 e-→ 2F (aq)
MnO, (aq) + 8 H*(aq) + 5 e
Cl2(8) + 2 e 2 CI (aq)
Cr,O,2 (aq) + 14 H*(aq) + 6 e 2 Cr*(aq) + 7 H20(0)
O2(g) + 4 H*(aq) + 4e 2 H2O(1)
Br2(1) + 2 e- 2 Br (aq)
NO3 (aq) + 4 H*(aq) + 3 e NO(g) + 2 H2O(1)
Ag*(aq) + e-
Fe* (aq) + e - Fe2*(aq)
O2(g) + 2 H*(aq) + 2 e H2O2(aq)
MnO, (aq) + 2 H20(1) + 3e - MnO2(s) + 4 OH (aq)
I2(s) + 2 e 21(aq)
O2(g) + 2 H2O(1) + 4e 4 OH (aq)
Cu²"(aq) + 2 e
2H*(aq) + 2 e¯ – H2(g)
Ni2*(aq) + 2 e
Fe2*(aq) + 2 e
Zn2*(aq) + 2 e
+2.87
+1.51
Mn2*(aq) + 4 H20(1)
+1.36
+1.33
+1.23
+1.06
+0.96
+0.80
Ag(s)
+0.77
+0.68
+0.59
+0.54
+0.40
+0.34
Cu(s)
-
0 [defined]
>
-0.28
Ni(s)
Fe(s)
-0.44
-0.76
Zn(s)
2 H2O(1) + 2e
Al3*(aq) + 3 e
Na*(aq) + e - Na(s)
Li*(aq) + e Li(s)
-0.83
H2(g) + 2 OH (aq)
Al(s)
-1.66
-2.71
-3.05
-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F29a20fd5-3cfb-4bcc-bf5f-6b441723c4e9%2F49577b9d-2a66-468c-aac8-689c8f54e0ce%2Fphj1xcb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:TABLE 18.1 Standard Reduction Potentials in Water at 25°C
Potential (V)
Reduction Half-Reaction
F2(g) + 2 e-→ 2F (aq)
MnO, (aq) + 8 H*(aq) + 5 e
Cl2(8) + 2 e 2 CI (aq)
Cr,O,2 (aq) + 14 H*(aq) + 6 e 2 Cr*(aq) + 7 H20(0)
O2(g) + 4 H*(aq) + 4e 2 H2O(1)
Br2(1) + 2 e- 2 Br (aq)
NO3 (aq) + 4 H*(aq) + 3 e NO(g) + 2 H2O(1)
Ag*(aq) + e-
Fe* (aq) + e - Fe2*(aq)
O2(g) + 2 H*(aq) + 2 e H2O2(aq)
MnO, (aq) + 2 H20(1) + 3e - MnO2(s) + 4 OH (aq)
I2(s) + 2 e 21(aq)
O2(g) + 2 H2O(1) + 4e 4 OH (aq)
Cu²"(aq) + 2 e
2H*(aq) + 2 e¯ – H2(g)
Ni2*(aq) + 2 e
Fe2*(aq) + 2 e
Zn2*(aq) + 2 e
+2.87
+1.51
Mn2*(aq) + 4 H20(1)
+1.36
+1.33
+1.23
+1.06
+0.96
+0.80
Ag(s)
+0.77
+0.68
+0.59
+0.54
+0.40
+0.34
Cu(s)
-
0 [defined]
>
-0.28
Ni(s)
Fe(s)
-0.44
-0.76
Zn(s)
2 H2O(1) + 2e
Al3*(aq) + 3 e
Na*(aq) + e - Na(s)
Li*(aq) + e Li(s)
-0.83
H2(g) + 2 OH (aq)
Al(s)
-1.66
-2.71
-3.05
-
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