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20. Electrochemistry

Cell Notation

20. Electrochemistry

Cell Notation

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The Cell Notation

The Cell Notation

Cell Notation Example

Cell Notation Example

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Multiple Choice

Write the half reactions as well as the overall net ionic equation for the following line notation:

Fe (s) | Fe²⁺(aq) || Mg²⁺(aq) | Mg (s)

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Multiple Choice

The cell notation for a redox reaction is given as the following at (T= 298 K). Calculate the cell potential for the reaction at 25ºC.

Zn (s) | Zn²⁺ (aq, 0.37 M) || Ni²⁺ (aq, 0.059 M) | Ni (s)

Standard Reduction Potentials

Zn²⁺ (aq) + 2 e^– →. Zn (s) E°_red = - 0.7621

Ni²⁺ (aq) + 2 e^– → Ni (s) E°_red = - 0.2300

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Multiple Choice

What is the [Cu²⁺] for the following cell notation diagram if the cell potential is 0.4404 V?

Cu | Cu²⁺ (aq, ? M) || Ag⁺(aq, 0.50 M) | Ag

Standard Reduction Potentials

Cu²⁺ (aq) + 2 e^– →. Cu (s) E°_red = + 0.3394

Ag⁺ (aq) + e^– → Ag (s) E°_red= + 0.8000

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Textbook Question

What is the line notation for the galvanic cell?

(a) (b) (c) (d)

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Textbook Question

What is the pH of the solution in the cathode compartment of the following cell if the measured cell potential at 25 °C is 0.58 V? (Refer to Appendix B for standard reduction potentials.) (a) 8.0 (b) 4.5 (c) 2.2 (d) 3.0

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Textbook Question

Use line notation to represent each electrochemical cell in Problem 43.

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Textbook Question

Make a sketch of the voltaic cell represented by the line nota- tion. Write the overall balanced equation for the reaction and calculate Ec°ell. Sn(s) | Sn2+(aq) || NO( g) | NO3-(aq), H+(aq) | Pt(s)

Has a video solution.

Textbook Question

Write a balanced equation for the overall cell reaction in the following galvanic cell, and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br-(aq) | Br2(l2) || Cl2(g) | Cl-(aq) || Pt(s)

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Textbook Question

Write the shorthand notation for a galvanic cell that uses the following cell reaction. Include inert electrodes if necessary. 2 Fe1s2 + Cr2O72-1aq2 + 14 H+1aq2¡2 Fe3+1aq2 + 2 Cr3+1aq2 + 7 H2O1l2

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Textbook Question

An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.

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Textbook Question

An H2/H+ half-cell (anode) and an Ag+/Ag half cell (cathode) are connected by a wire and a salt bridge. (c) Give the shorthand notation for the cell.

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Textbook Question

Write balanced equations for the electrode and overall cell reactions in the following galvanic cells. Sketch each cell, labeling the anode and cathode and showing the direction of electron and ion flow. (a) .

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Textbook Question

The standard potential for the following galvanic cell is 0.40 V: (Europium, Eu, is one of the lanthanide elements.) Use the data in Table 19.1 to calculate the standard reduction potential for Eu3+/Eu2+ half-cell.

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Textbook Question

What is the Fe2+: Sn2+ concentration ratio in the following cell at 25 °C if the measured cell potential is 0.35 V?

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Textbook Question

What is the pH of the solution in the cathode compartment of the following cell if the measured cell potential at 25 °C is 0.17 V?

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Textbook Question

The cell potential of this electrochemical cell depends on the pH of the solution in the anode half-cell. Pt(s) | H2(g, 1 atm) | H+(aq, ? M) || Cu2+(aq, 1.0 M) | Cu(s) What is the pH of the solution if Ecell is 355 mV?

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Textbook Question

The cell potential of this electrochemical cell depends on the gold concentration in the cathode half-cell. Pt(s) | H2(g, 1.0 atm) | H+(aq, 1.0 M) || Au3+(aq, ? M) | Au(s) What is the concentration of Au3+ in the solution if Ecell is 1.22 V?

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Textbook Question

The following galvanic cell has a potential of 1.214 V at 25 °C: Calculate the value of Ksp for Hg2Br2 at 25°C

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For the following electrochemical cell

Cu(s) | Cu₂(aq, 0.0155 m) || Ag(aq, 2.50 m) | Ag(s)

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What is the balanced reaction for the cell diagram below? Al(s) | Al³⁺(aq) || Cd²⁺(aq) | Cd(s)

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