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calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given. H2O (l) <=> H+ (aq) + OH- (aq)

calculate equilibrium constants for the following reactions. Assume 298.15 K if no temperature is given. H2O (l) <=> H+ (aq) + OH- (aq)

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 99QAP: The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another...
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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.
H2O (l) <=> H+ (aq) + OH- (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 -
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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