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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
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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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 | |---------------|--------------------------------------------------------------| | +2.87 | \( \text{F}_2(g) + 2e^- \rightarrow 2 \text{F}^-(aq) \) | | +1.51 | \( \text{MnO}_4^-(aq) + 8 \text{H}^+(aq) + 5e^- \rightarrow \text{Mn}^{2+}(aq) + 4 \text{H}_2\text{O}(l) \) | | +1.36 | \( \text{Cl}_2(g) + 2e^- \rightarrow 2 \text{Cl}^-(aq) \) | | +1.33 | \( \text{Cr}_2\text{O}_7^{2-}(aq) + 14 \text{H}^+(aq) + 6e^- \rightarrow 2 \text{Cr}^{3+}(aq) + 7 \text{H}_2\text{O}(l) \) | | +1.23 | \( \text{O}_2(g) + 4 \text{H}^+(aq) + 4e^- \rightarrow 2 \text{H}_2\text{O}(l) \) | | +1.06 | \( \text{Br}_2(l) + 2e^- \rightarrow 2 \text{Br}^-(aq) \) | | +0.96 | \( \text{NO}_3^-(aq) + 4 \text{H}^+(aq) + 3e^- \rightarrow \text{NO}(g) + 2 \text{H}_2\text{O}(l) \) | | +0.80 | \( \text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s) \) | | +0.77 | \( \text{Fe}^{3+}(aq) + e^- \rightarrow \text{Fe}^{2+}(aq) \)| | +0.68 | \( \text{O}_2(g) + 2 \text{
Transcribed Image Text:**Table 18.1: Standard Reduction Potentials in Water at 25°C** | Potential (V) | Reduction Half-Reaction | |---------------|--------------------------------------------------------------| | +2.87 | \( \text{F}_2(g) + 2e^- \rightarrow 2 \text{F}^-(aq) \) | | +1.51 | \( \text{MnO}_4^-(aq) + 8 \text{H}^+(aq) + 5e^- \rightarrow \text{Mn}^{2+}(aq) + 4 \text{H}_2\text{O}(l) \) | | +1.36 | \( \text{Cl}_2(g) + 2e^- \rightarrow 2 \text{Cl}^-(aq) \) | | +1.33 | \( \text{Cr}_2\text{O}_7^{2-}(aq) + 14 \text{H}^+(aq) + 6e^- \rightarrow 2 \text{Cr}^{3+}(aq) + 7 \text{H}_2\text{O}(l) \) | | +1.23 | \( \text{O}_2(g) + 4 \text{H}^+(aq) + 4e^- \rightarrow 2 \text{H}_2\text{O}(l) \) | | +1.06 | \( \text{Br}_2(l) + 2e^- \rightarrow 2 \text{Br}^-(aq) \) | | +0.96 | \( \text{NO}_3^-(aq) + 4 \text{H}^+(aq) + 3e^- \rightarrow \text{NO}(g) + 2 \text{H}_2\text{O}(l) \) | | +0.80 | \( \text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s) \) | | +0.77 | \( \text{Fe}^{3+}(aq) + e^- \rightarrow \text{Fe}^{2+}(aq) \)| | +0.68 | \( \text{O}_2(g) + 2 \text{
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