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A galvanic cell is set up to operate with the half-reactions: Co3+ + 3 e- → Co Au3+ + 3 e- → Au a) How many electrons are exchanged in the electrochemical reaction that follows? b) What is Eo of the reaction in V? c) What is ∆Go of the reaction in kJ/mol?

A galvanic cell is set up to operate with the half-reactions: Co3+ + 3 e- → Co Au3+ + 3 e- → Au a) How many electrons are exchanged in the electrochemical reaction that follows? b) What is Eo of the reaction in V? c) What is ∆Go of the reaction in kJ/mol?

Chemistry
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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
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A galvanic cell is set up to operate with the half-reactions:

Co3+ + 3 e- → Co
Au3+ + 3 e- → Au


a) How many electrons are exchanged in the electrochemical reaction that follows?


b) What is Eo of the reaction in V?

c) What is ∆Go of the reaction in kJ/mol?

Here is the transcription of the table for an educational website: --- ### Standard Reduction Potentials Table The following table lists various half-reactions along with their standard reduction potentials (E°) measured in volts (V). These values are crucial in understanding the relative tendency of different substances to gain electrons and undergo reduction. | Half-Reaction | E° (V) | |----------------------------------------|-------| | Co³⁺ + 3 e⁻ → Co | 1.82 | | MnO₄⁻ + 4 H⁺ + 3 e⁻ → MnO₂ + 2 H₂O | 1.68 | | Au³⁺ + 3 e⁻ → Au | 1.5 | | O₂ + 4 H⁺ + 4 e⁻ → 2 H₂O | 1.23 | | NO₃⁻ + 4 H⁺ + 3 e⁻ → NO + 2 H₂O | 0.96 | | Ag⁺ + e⁻ → Ag | 0.8 | | Cu²⁺ + 2 e⁻ → Cu | 0.52 | | SO₄²⁻ + 4 H⁺ + 2 e⁻ → H₂SO₃ + H₂O | 0.2 | | Ni²⁺ + 2 e⁻ → Ni | -0.23 | | Cr³⁺ + 3 e⁻ → Cr²⁺ | -0.41 | | 2 H₂O + 2 e⁻ → H₂ + 2 OH⁻ | -0.83 | | Mn²⁺ + 2 e⁻ → Mn | -1.18 | | Ca²⁺ + 2 e⁻ → Ca | -2.76 | **Explanation of Terms:** - **Half-Reaction**: A reaction that shows either the reduction or oxidation process separately. - **Reduction Potential (E°)**: The tendency of a chemical species to gain electrons and thereby get reduced. A higher E° value indicates a greater tendency to gain electrons. These standard reduction potentials are measured under standard conditions: 25°C, 1 M concentration for each ion participating in the reaction, and a partial
Transcribed Image Text:Here is the transcription of the table for an educational website: --- ### Standard Reduction Potentials Table The following table lists various half-reactions along with their standard reduction potentials (E°) measured in volts (V). These values are crucial in understanding the relative tendency of different substances to gain electrons and undergo reduction. | Half-Reaction | E° (V) | |----------------------------------------|-------| | Co³⁺ + 3 e⁻ → Co | 1.82 | | MnO₄⁻ + 4 H⁺ + 3 e⁻ → MnO₂ + 2 H₂O | 1.68 | | Au³⁺ + 3 e⁻ → Au | 1.5 | | O₂ + 4 H⁺ + 4 e⁻ → 2 H₂O | 1.23 | | NO₃⁻ + 4 H⁺ + 3 e⁻ → NO + 2 H₂O | 0.96 | | Ag⁺ + e⁻ → Ag | 0.8 | | Cu²⁺ + 2 e⁻ → Cu | 0.52 | | SO₄²⁻ + 4 H⁺ + 2 e⁻ → H₂SO₃ + H₂O | 0.2 | | Ni²⁺ + 2 e⁻ → Ni | -0.23 | | Cr³⁺ + 3 e⁻ → Cr²⁺ | -0.41 | | 2 H₂O + 2 e⁻ → H₂ + 2 OH⁻ | -0.83 | | Mn²⁺ + 2 e⁻ → Mn | -1.18 | | Ca²⁺ + 2 e⁻ → Ca | -2.76 | **Explanation of Terms:** - **Half-Reaction**: A reaction that shows either the reduction or oxidation process separately. - **Reduction Potential (E°)**: The tendency of a chemical species to gain electrons and thereby get reduced. A higher E° value indicates a greater tendency to gain electrons. These standard reduction potentials are measured under standard conditions: 25°C, 1 M concentration for each ion participating in the reaction, and a partial
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