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V Porous Barrier Al 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.

V Porous Barrier Al 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.

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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### Standard Reduction Potentials Table The table below lists standard reduction potentials (E°) for various redox couples, expressed in volts. These values indicate the tendency of a species to gain electrons (undergo reduction) under standard conditions (25°C, 1 M concentration, and 1 atm pressure). Positive values represent a greater tendency to be reduced. **Couple** | **E° (Volts)** --- | --- F₂ / HF (H⁺) | +3.03 F₂ / F⁻ | +2.87 S₂O₈²⁻ / SO₄²⁻ | +2.05 BiO₃⁻ / Bi³⁺ | +2.0 H₂O₂ / H₂O (H⁺) | +1.78 PbO₂ / PbSO₄ (H⁺, SO₄²⁻) | +1.685 Ce⁴⁺ / Ce³⁺ | +1.61 MnO₄⁻ / Mn²⁺ (H⁺) | +1.491 ClO₃⁻ / Cl⁻ (H⁺) | +1.47 PbO₂ / Pb²⁺ (H⁺) | +1.46 Au³⁺ / Au | +1.42 Cl₂ / Cl⁻ | +1.358 Cr₂O₇²⁻ / Cr³⁺ (H⁺) | +1.33 MnO₂ / Mn²⁺ (H⁺) | +1.28 O₂ / H₂O₂ (H⁺) | +1.229 Br₂ / Br⁻ | +1.065 NO₃⁻ / NO (H⁺) | +0.96 Hg₂²⁺ / Hg₂²⁺ | +0.910 H₂O₂ / OH⁻ | +0.87 O₂ / H₂O (pH = 7) | +0.82 Ag⁺ / Ag | +0.7996 Hg₂²⁺ / Hg | +0.799 Fe³⁺ / Fe²⁺ | +0.771 H₂O₂ / H₂O (H⁺) | +0.682
Transcribed Image Text:### Standard Reduction Potentials Table The table below lists standard reduction potentials (E°) for various redox couples, expressed in volts. These values indicate the tendency of a species to gain electrons (undergo reduction) under standard conditions (25°C, 1 M concentration, and 1 atm pressure). Positive values represent a greater tendency to be reduced. **Couple** | **E° (Volts)** --- | --- F₂ / HF (H⁺) | +3.03 F₂ / F⁻ | +2.87 S₂O₈²⁻ / SO₄²⁻ | +2.05 BiO₃⁻ / Bi³⁺ | +2.0 H₂O₂ / H₂O (H⁺) | +1.78 PbO₂ / PbSO₄ (H⁺, SO₄²⁻) | +1.685 Ce⁴⁺ / Ce³⁺ | +1.61 MnO₄⁻ / Mn²⁺ (H⁺) | +1.491 ClO₃⁻ / Cl⁻ (H⁺) | +1.47 PbO₂ / Pb²⁺ (H⁺) | +1.46 Au³⁺ / Au | +1.42 Cl₂ / Cl⁻ | +1.358 Cr₂O₇²⁻ / Cr³⁺ (H⁺) | +1.33 MnO₂ / Mn²⁺ (H⁺) | +1.28 O₂ / H₂O₂ (H⁺) | +1.229 Br₂ / Br⁻ | +1.065 NO₃⁻ / NO (H⁺) | +0.96 Hg₂²⁺ / Hg₂²⁺ | +0.910 H₂O₂ / OH⁻ | +0.87 O₂ / H₂O (pH = 7) | +0.82 Ag⁺ / Ag | +0.7996 Hg₂²⁺ / Hg | +0.799 Fe³⁺ / Fe²⁺ | +0.771 H₂O₂ / H₂O (H⁺) | +0.682
### Using the Voltaic Cell #### A) Write the equation for this cell. #### B) Calculate standard cell potential (E°). #### C) Calculate the voltage for this cell. #### D) Labeling the Diagram In the above diagram, label the anode, cathode and draw an arrow showing the flow of electrons in the cell. **Diagram Explanation:** The diagram shows a voltaic (or galvanic) cell consisting of two half-cells connected by a porous barrier. On the left side, there is an aluminum (Al) electrode immersed in a 0.435 M Al³⁺ solution, and on the right side, there is a tin (Sn) electrode immersed in a 0.00212 M Sn²⁺ solution. A voltmeter (denoted by "V") is connected between the two electrodes to measure the voltage of the cell. The porous barrier allows ions to flow between the two half-cells to maintain charge balance. **Components:** - **Aluminum Electrode (left):** Labeled "Al," it is placed in a 0.435 M solution of aluminum ions (Al³⁺). - **Tin Electrode (right):** Labeled "Sn," it is placed in a 0.00212 M solution of tin ions (Sn²⁺). - **Porous Barrier:** Located between the two solutions to allow ion exchange. - **Voltmeter (V):** Measures the voltage difference between the two electrodes. #### E) Write the cell diagram. --- This educational content helps students understand how to write cell equations, calculate standard cell potentials, calculate cell voltages, and correctly label and interpret a voltaic cell diagram.
Transcribed Image Text:### Using the Voltaic Cell #### A) Write the equation for this cell. #### B) Calculate standard cell potential (E°). #### C) Calculate the voltage for this cell. #### D) Labeling the Diagram In the above diagram, label the anode, cathode and draw an arrow showing the flow of electrons in the cell. **Diagram Explanation:** The diagram shows a voltaic (or galvanic) cell consisting of two half-cells connected by a porous barrier. On the left side, there is an aluminum (Al) electrode immersed in a 0.435 M Al³⁺ solution, and on the right side, there is a tin (Sn) electrode immersed in a 0.00212 M Sn²⁺ solution. A voltmeter (denoted by "V") is connected between the two electrodes to measure the voltage of the cell. The porous barrier allows ions to flow between the two half-cells to maintain charge balance. **Components:** - **Aluminum Electrode (left):** Labeled "Al," it is placed in a 0.435 M solution of aluminum ions (Al³⁺). - **Tin Electrode (right):** Labeled "Sn," it is placed in a 0.00212 M solution of tin ions (Sn²⁺). - **Porous Barrier:** Located between the two solutions to allow ion exchange. - **Voltmeter (V):** Measures the voltage difference between the two electrodes. #### E) Write the cell diagram. --- This educational content helps students understand how to write cell equations, calculate standard cell potentials, calculate cell voltages, and correctly label and interpret a voltaic cell diagram.
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