Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid: 2Fe³+ + 2I- = 2FE²+ +I_(aq) See appendix H in the textbook for standard reduction potentials.

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**Appendix H: Standard Reduction Potentials**

This table presents standard reduction potentials for various chemical reactions, each with their respective electrochemical cell notation and potential values. These potentials are presented in volts (E°) and are measured under standard conditions. The table provides essential data for understanding redox reactions in electrochemical cells.

---

**Table Columns:**

1. **Reaction:** Displays the chemical equation for the reduction process.
2. **E° (volts):** Lists the standard reduction potential for each reaction, indicating the tendency of a species to be reduced.
3. **ΔE°/T (mV/K):** Provides the temperature coefficient of the potential, representing how the potential changes with temperature.

---

**Selected Entries:**

- **Dysprosium**
  - Dy³⁺ + 3e⁻ → Dy(s): E° = -2.295 V, ΔE°/T = 0.073 mV/K

- **Europium**
  - Eu³⁺ + 3e⁻ → Eu(s): E° = -1.991 V, ΔE°/T = 0.058 mV/K

- **Fluorine**
  - F₂(g) + 2e⁻ → 2F⁻: E° = 2.812 V, ΔE°/T = -0.126 mV/K

- **Gold**
  - Au⁺ + e⁻ → Au(s): E° = 1.69 V, ΔE°/T = -0.1 mV/K

- **Iron (Fe³⁺/Fe²⁺)**
  - Fe³⁺ + e⁻ → Fe²⁺: E° = 0.77 V, ΔE°/T = 1.175 mV/K

---

These reduction potentials play a crucial role in determining the direction of electron flow in electrochemical cells and are fundamental in calculating Gibbs free energy changes in redox reactions. Understanding them is essential for various applications, including batteries, corrosion prevention, and electroplating.

**Notes:**
- The conditions, such as the concentration of ions and pressure, should be standard (usually 1M concentration and 1 atm pressure).
- Negative potentials indicate a lesser tendency to be reduced compared to hydrogen, whereas positive potentials suggest a greater tendency.

This table forms an essential resource for students and professionals
Transcribed Image Text:**Appendix H: Standard Reduction Potentials** This table presents standard reduction potentials for various chemical reactions, each with their respective electrochemical cell notation and potential values. These potentials are presented in volts (E°) and are measured under standard conditions. The table provides essential data for understanding redox reactions in electrochemical cells. --- **Table Columns:** 1. **Reaction:** Displays the chemical equation for the reduction process. 2. **E° (volts):** Lists the standard reduction potential for each reaction, indicating the tendency of a species to be reduced. 3. **ΔE°/T (mV/K):** Provides the temperature coefficient of the potential, representing how the potential changes with temperature. --- **Selected Entries:** - **Dysprosium** - Dy³⁺ + 3e⁻ → Dy(s): E° = -2.295 V, ΔE°/T = 0.073 mV/K - **Europium** - Eu³⁺ + 3e⁻ → Eu(s): E° = -1.991 V, ΔE°/T = 0.058 mV/K - **Fluorine** - F₂(g) + 2e⁻ → 2F⁻: E° = 2.812 V, ΔE°/T = -0.126 mV/K - **Gold** - Au⁺ + e⁻ → Au(s): E° = 1.69 V, ΔE°/T = -0.1 mV/K - **Iron (Fe³⁺/Fe²⁺)** - Fe³⁺ + e⁻ → Fe²⁺: E° = 0.77 V, ΔE°/T = 1.175 mV/K --- These reduction potentials play a crucial role in determining the direction of electron flow in electrochemical cells and are fundamental in calculating Gibbs free energy changes in redox reactions. Understanding them is essential for various applications, including batteries, corrosion prevention, and electroplating. **Notes:** - The conditions, such as the concentration of ions and pressure, should be standard (usually 1M concentration and 1 atm pressure). - Negative potentials indicate a lesser tendency to be reduced compared to hydrogen, whereas positive potentials suggest a greater tendency. This table forms an essential resource for students and professionals
**Equilibrium Constant Calculation for Redox Reaction in Perchloric Acid**

**Objective:**
Calculate the equilibrium constant (K_eq) for the redox reaction carried out in 1 M perchloric acid.

**Reaction:**
\[ 2\text{Fe}^{3+} + 2\text{I}^- \rightleftharpoons 2\text{Fe}^{2+} + \text{I}_2(\text{aq}) \]

**Procedure:**
To find the equilibrium constant for the reaction, refer to Appendix H in the textbook for the standard reduction potentials. Use the Nernst equation and the relationship between Gibbs free energy and the equilibrium constant.

**Note:**
Understanding the standard reduction potentials will help in calculating the cell potential, and subsequently the equilibrium constant.
Transcribed Image Text:**Equilibrium Constant Calculation for Redox Reaction in Perchloric Acid** **Objective:** Calculate the equilibrium constant (K_eq) for the redox reaction carried out in 1 M perchloric acid. **Reaction:** \[ 2\text{Fe}^{3+} + 2\text{I}^- \rightleftharpoons 2\text{Fe}^{2+} + \text{I}_2(\text{aq}) \] **Procedure:** To find the equilibrium constant for the reaction, refer to Appendix H in the textbook for the standard reduction potentials. Use the Nernst equation and the relationship between Gibbs free energy and the equilibrium constant. **Note:** Understanding the standard reduction potentials will help in calculating the cell potential, and subsequently the equilibrium constant.
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