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**Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C** This table provides the standard electrode potentials, \( E^\circ \), for various half-reactions at 25°C, commonly used in electrochemistry. The potentials are measured in volts (V), indicating the ability of each species to acquire electrons (get reduced). | **Cathode (Reduction) Half-Reaction** | **Standard Potential, \( E^\circ \) (Volts)** | |---------------------------------------|---------------------------------------------| | \( \text{Li}^+(\text{aq}) + e^- \rightarrow \text{Li}(\text{s}) \) | -3.04 | | \( \text{K}^+(\text{aq}) + e^- \rightarrow \text{K}(\text{s}) \) | -2.92 | | \( \text{Ca}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Ca}(\text{s}) \) | -2.76 | | \( \text{Na}^+(\text{aq}) + e^- \rightarrow \text{Na}(\text{s}) \) | -2.71 | | \( \text{Mg}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Mg}(\text{s}) \) | -2.38 | | \( \text{Al}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Al}(\text{s}) \) | -1.66 | | \( 2\text{H}_2\text{O}(\text{l}) + 2e^- \rightarrow \text{H}_2(\text{g}) + 2\text{OH}^-(\text{aq}) \) | -0.83 | | \( \text{Zn}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Zn}(\text{s}) \) | -0.76 | | \( \text{Cr}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Cr}(\text{s}) \) | -0.74 | | \( \text{Fe}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Fe}(\text{s

**Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C** This table provides the standard electrode potentials, \( E^\circ \), for various half-reactions at 25°C, commonly used in electrochemistry. The potentials are measured in volts (V), indicating the ability of each species to acquire electrons (get reduced). | **Cathode (Reduction) Half-Reaction** | **Standard Potential, \( E^\circ \) (Volts)** | |---------------------------------------|---------------------------------------------| | \( \text{Li}^+(\text{aq}) + e^- \rightarrow \text{Li}(\text{s}) \) | -3.04 | | \( \text{K}^+(\text{aq}) + e^- \rightarrow \text{K}(\text{s}) \) | -2.92 | | \( \text{Ca}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Ca}(\text{s}) \) | -2.76 | | \( \text{Na}^+(\text{aq}) + e^- \rightarrow \text{Na}(\text{s}) \) | -2.71 | | \( \text{Mg}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Mg}(\text{s}) \) | -2.38 | | \( \text{Al}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Al}(\text{s}) \) | -1.66 | | \( 2\text{H}_2\text{O}(\text{l}) + 2e^- \rightarrow \text{H}_2(\text{g}) + 2\text{OH}^-(\text{aq}) \) | -0.83 | | \( \text{Zn}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Zn}(\text{s}) \) | -0.76 | | \( \text{Cr}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Cr}(\text{s}) \) | -0.74 | | \( \text{Fe}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Fe}(\text{s

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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  1. Calculate ΔG° (kJ) for the reaction Hg(l) + S2-(aq)  + 2Ag+(aq)  →  Ag(s)  + HgS(s)  using the tabluated electrode potentials. Use the equation ΔG°=-nFΔE° 
    Faraday constant= 96500C/mol e-
    J = C x V
**Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C** This table provides the standard electrode potentials, \( E^\circ \), for various half-reactions at 25°C, commonly used in electrochemistry. The potentials are measured in volts (V), indicating the ability of each species to acquire electrons (get reduced). | **Cathode (Reduction) Half-Reaction** | **Standard Potential, \( E^\circ \) (Volts)** | |---------------------------------------|---------------------------------------------| | \( \text{Li}^+(\text{aq}) + e^- \rightarrow \text{Li}(\text{s}) \) | -3.04 | | \( \text{K}^+(\text{aq}) + e^- \rightarrow \text{K}(\text{s}) \) | -2.92 | | \( \text{Ca}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Ca}(\text{s}) \) | -2.76 | | \( \text{Na}^+(\text{aq}) + e^- \rightarrow \text{Na}(\text{s}) \) | -2.71 | | \( \text{Mg}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Mg}(\text{s}) \) | -2.38 | | \( \text{Al}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Al}(\text{s}) \) | -1.66 | | \( 2\text{H}_2\text{O}(\text{l}) + 2e^- \rightarrow \text{H}_2(\text{g}) + 2\text{OH}^-(\text{aq}) \) | -0.83 | | \( \text{Zn}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Zn}(\text{s}) \) | -0.76 | | \( \text{Cr}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Cr}(\text{s}) \) | -0.74 | | \( \text{Fe}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Fe}(\text{s
Transcribed Image Text:**Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C** This table provides the standard electrode potentials, \( E^\circ \), for various half-reactions at 25°C, commonly used in electrochemistry. The potentials are measured in volts (V), indicating the ability of each species to acquire electrons (get reduced). | **Cathode (Reduction) Half-Reaction** | **Standard Potential, \( E^\circ \) (Volts)** | |---------------------------------------|---------------------------------------------| | \( \text{Li}^+(\text{aq}) + e^- \rightarrow \text{Li}(\text{s}) \) | -3.04 | | \( \text{K}^+(\text{aq}) + e^- \rightarrow \text{K}(\text{s}) \) | -2.92 | | \( \text{Ca}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Ca}(\text{s}) \) | -2.76 | | \( \text{Na}^+(\text{aq}) + e^- \rightarrow \text{Na}(\text{s}) \) | -2.71 | | \( \text{Mg}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Mg}(\text{s}) \) | -2.38 | | \( \text{Al}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Al}(\text{s}) \) | -1.66 | | \( 2\text{H}_2\text{O}(\text{l}) + 2e^- \rightarrow \text{H}_2(\text{g}) + 2\text{OH}^-(\text{aq}) \) | -0.83 | | \( \text{Zn}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Zn}(\text{s}) \) | -0.76 | | \( \text{Cr}^{3+}(\text{aq}) + 3e^- \rightarrow \text{Cr}(\text{s}) \) | -0.74 | | \( \text{Fe}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Fe}(\text{s
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