Using the half reaction data in (Table 9.3), write balanced overall reactions for the following redox processes. Calculate the E⁰, pe⁰ and ΔG⁰ values for each overall reaction. Indicate whether each reaction is thermodynamically favorable under standard conditions.i) Oxidation of Mn²⁺ to MnO₂(s) using I₂(aq) to form I⁻.ii) Oxidation of Pb(s) to Pb²⁺ by Zn²⁺ to form Zn(s). Below is a transcription and explanation of the chemical equilibrium data from the provided image. This content is suitable for an educational setting, focusing on chemistry.### Chemical Equilibrium ConstantsThe table presents a series of chemical reactions, along with their respective equilibrium constants (Log K), standard electrode potentials (pe°), and reduction potentials (E° in mV). These values are critical in understanding the behavior of reactions in various conditions and can be used to predict reaction spontaneity and direction.#### Key- **Reaction**: Represents the chemical equation for the transformation being studied.- **Log K**: The logarithm of the equilibrium constant, providing insights into the favorability of a reaction at standard conditions.- **pe°**: The standard electron potential, indicating the tendency of a substance to gain or lose electrons.- **E° (mV)**: The standard reduction potential in millivolts, which also provides similar information to pe°.#### Sample Reactions and Their Values1. **NO₃⁻ + 2e⁻ + 2H⁺ ↔ NO₂⁻ + H₂O** - Log K: 28.57 - pe°: 3.63 - E° (mV): 4212. **NO₃⁻ + 10e⁻ + 10H⁺ ↔ NH₄⁺ + 3H₂O** - Log K: 110.98 - pe°: 8.06 - E° (mV): 13483. **Cr₂O₇²⁻ + 6e⁻ + 14H⁺ ↔ 2Cr³⁺ + 7H₂O** - Log K: 130.94 - pe°: 8.18 - E° (mV): 13924. **Fe³⁺ + e⁻ ↔ Fe²⁺** - Log K: 15.04 - pe°: 1.31 - E° (mV): 7715. **O₂(g) + 4e⁻ + 4H⁺ ↔ 2H₂O** - Log K: 83.01 - pe°: 5.80 - E° (m

Given Redox process: To Calculate: Calculate the E0, pe0 and ∆G0 values for each overall reaction.

Using the half reaction data in (Table 9.3; write balanced overall reactions for the following redox processes. Calculate the Eº, pe° and AG values for each overall reaction. Indicate whether each reaction is thermodynamically favorable under standard conditions.

Using the half reaction data in (Table 9.3; write balanced overall reactions for the following redox processes. Calculate the Eº, pe° and AG values for each overall reaction. Indicate whether each reaction is thermodynamically favorable under standard conditions.

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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Question

100%

Using the half reaction data in (Table 9.3), write balanced overall reactions for the following redox processes. Calculate the E⁰, pe⁰ and ΔG⁰ values for each overall reaction. Indicate whether each reaction is thermodynamically favorable under standard conditions.

i) Oxidation of Mn²⁺ to MnO₂(s) using I₂(aq) to form I⁻.
ii) Oxidation of Pb(s) to Pb²⁺ by Zn²⁺ to form Zn(s).

Below is a transcription and explanation of the chemical equilibrium data from the provided image. This content is suitable for an educational setting, focusing on chemistry.

### Chemical Equilibrium Constants

The table presents a series of chemical reactions, along with their respective equilibrium constants (Log K), standard electrode potentials (pe°), and reduction potentials (E° in mV). These values are critical in understanding the behavior of reactions in various conditions and can be used to predict reaction spontaneity and direction.

#### Key

- **Reaction**: Represents the chemical equation for the transformation being studied.
- **Log K**: The logarithm of the equilibrium constant, providing insights into the favorability of a reaction at standard conditions.
- **pe°**: The standard electron potential, indicating the tendency of a substance to gain or lose electrons.
- **E° (mV)**: The standard reduction potential in millivolts, which also provides similar information to pe°.

#### Sample Reactions and Their Values

1. **NO₃⁻ + 2e⁻ + 2H⁺ ↔ NO₂⁻ + H₂O**
- Log K: 28.57
- pe°: 3.63
- E° (mV): 421

2. **NO₃⁻ + 10e⁻ + 10H⁺ ↔ NH₄⁺ + 3H₂O**
- Log K: 110.98
- pe°: 8.06
- E° (mV): 1348

3. **Cr₂O₇²⁻ + 6e⁻ + 14H⁺ ↔ 2Cr³⁺ + 7H₂O**
- Log K: 130.94
- pe°: 8.18
- E° (mV): 1392

4. **Fe³⁺ + e⁻ ↔ Fe²⁺**
- Log K: 15.04
- pe°: 1.31
- E° (mV): 771

5. **O₂(g) + 4e⁻ + 4H⁺ ↔ 2H₂O**
- Log K: 83.01
- pe°: 5.80
- E° (m

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