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V Porous Barrier AI Sn 0.435 M AI3+ 0.00212 M Sn2+ D. In the above diagram, label the anode, cathode and draw an arrow showing the flow of electrons in the cell. E. Write the cell diagram.

V Porous Barrier AI Sn 0.435 M AI3+ 0.00212 M Sn2+ D. In the above diagram, label the anode, cathode and draw an arrow showing the flow of electrons in the cell. E. Write the cell diagram.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.24QP: Electrochemical Cells II Consider this cell running under standard conditions:...
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# Standard Reduction Potentials Chart The table below lists the standard reduction potentials (E°) for various chemical species. These values are measured in volts under standard conditions (1M concentration, 25°C, 1 atm pressure) relative to the standard hydrogen electrode, which is assigned a potential of 0.00 volts. ## Standard Reduction Potentials | **Couple** | | **E° (Volts)** | | **Couple** | | **E° (Volts)** | |----------------|--|----------------|--|--------------|--|----------------| | F₂ | → | HF (H⁺) | = | +3.03 | | SO₄²⁻ | → | H₂SO₃ (H⁺) | = | +0.20 | | F₂ | → | F⁻ | = | +2.87 | | Sn⁴⁺ | → | Sn²⁺ | = | +0.15 | | S₂O₈²⁻ | → | SO₄²⁻ | = | +2.05 | | S | → | H₂S (H⁺) | = | +0.141 | | BiO₃⁻ | → | Bi³⁺ | = | +2.0 | | Hg₂Br₂ | → | Hg (Br⁻) | = | +0.140 | | H₂O₂ | → | H₂O (H⁺) | = | +1.78 | | AgBr | → | Ag (Br⁻) | = | +0.0713 | | PbO₂ | → | PbSO₄ (H⁺, SO₄²⁻) | = | +1.685 | | H⁺ | → | H₂ | = | +0.0000 | | Ce⁴⁺ | → | Ce³⁺ | = | +1.61 | | Pb²⁺ | → | Pb | = | -0.126 | | MnO
Transcribed Image Text:# Standard Reduction Potentials Chart The table below lists the standard reduction potentials (E°) for various chemical species. These values are measured in volts under standard conditions (1M concentration, 25°C, 1 atm pressure) relative to the standard hydrogen electrode, which is assigned a potential of 0.00 volts. ## Standard Reduction Potentials | **Couple** | | **E° (Volts)** | | **Couple** | | **E° (Volts)** | |----------------|--|----------------|--|--------------|--|----------------| | F₂ | → | HF (H⁺) | = | +3.03 | | SO₄²⁻ | → | H₂SO₃ (H⁺) | = | +0.20 | | F₂ | → | F⁻ | = | +2.87 | | Sn⁴⁺ | → | Sn²⁺ | = | +0.15 | | S₂O₈²⁻ | → | SO₄²⁻ | = | +2.05 | | S | → | H₂S (H⁺) | = | +0.141 | | BiO₃⁻ | → | Bi³⁺ | = | +2.0 | | Hg₂Br₂ | → | Hg (Br⁻) | = | +0.140 | | H₂O₂ | → | H₂O (H⁺) | = | +1.78 | | AgBr | → | Ag (Br⁻) | = | +0.0713 | | PbO₂ | → | PbSO₄ (H⁺, SO₄²⁻) | = | +1.685 | | H⁺ | → | H₂ | = | +0.0000 | | Ce⁴⁺ | → | Ce³⁺ | = | +1.61 | | Pb²⁺ | → | Pb | = | -0.126 | | MnO
**Using the voltaic cell below:** **A) Write the equation for this cell.** **B) Calculate standard cell potential (E°).** **C) Calculate the voltage for this cell.** --- **Diagram Explanation:** The diagram shows a voltaic cell setup with two half-cells. - The left half-cell consists of an aluminum (Al) electrode immersed in a solution with a concentration of 0.435 M of \( Al^{3+} \) ions. - The right half-cell consists of a tin (Sn) electrode immersed in a solution with a concentration of 0.00212 M of \( Sn^{2+} \) ions. - There is a porous barrier between the two half-cells which allows ionic movement while keeping the solutions separate. - A voltmeter (V) is connected between the two electrodes to measure the cell potential. **D) In the above diagram, label the anode, cathode and draw an arrow showing the flow of electrons in the cell.** **E) Write the cell diagram.** --- **Guidelines for Labeling and Writing Cell Diagram:** - **Anode**: The electrode where oxidation occurs. Typically, it's the more negative electrode or the one losing electrons. - **Cathode**: The electrode where reduction occurs. Typically, it's the more positive electrode or the one gaining electrons. - **Electron flow**: Electrons flow from the anode to the cathode through the external circuit. **Example of Cell Diagram Notation:** Al(s) | \( Al^{3+} \) (0.435 M) || \( Sn^{2+} \) (0.00212 M) | Sn(s)
Transcribed Image Text:**Using the voltaic cell below:** **A) Write the equation for this cell.** **B) Calculate standard cell potential (E°).** **C) Calculate the voltage for this cell.** --- **Diagram Explanation:** The diagram shows a voltaic cell setup with two half-cells. - The left half-cell consists of an aluminum (Al) electrode immersed in a solution with a concentration of 0.435 M of \( Al^{3+} \) ions. - The right half-cell consists of a tin (Sn) electrode immersed in a solution with a concentration of 0.00212 M of \( Sn^{2+} \) ions. - There is a porous barrier between the two half-cells which allows ionic movement while keeping the solutions separate. - A voltmeter (V) is connected between the two electrodes to measure the cell potential. **D) In the above diagram, label the anode, cathode and draw an arrow showing the flow of electrons in the cell.** **E) Write the cell diagram.** --- **Guidelines for Labeling and Writing Cell Diagram:** - **Anode**: The electrode where oxidation occurs. Typically, it's the more negative electrode or the one losing electrons. - **Cathode**: The electrode where reduction occurs. Typically, it's the more positive electrode or the one gaining electrons. - **Electron flow**: Electrons flow from the anode to the cathode through the external circuit. **Example of Cell Diagram Notation:** Al(s) | \( Al^{3+} \) (0.435 M) || \( Sn^{2+} \) (0.00212 M) | Sn(s)
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