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Ch.19 - Electrochemistry
All textbooksTro 4th EditionCh.19 - ElectrochemistryProblem 46
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Chapter 19, Problem 46

Calculate the standard cell potential for each of the electrochemical cells in Problem 44.

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1
Identify the half-reactions involved in the electrochemical cell from Problem 44.
Write the reduction half-reaction and its standard reduction potential, E° (from a standard reduction potential table).
Write the oxidation half-reaction and its standard reduction potential, E° (from a standard reduction potential table).
Calculate the standard cell potential, E°_cell, using the formula: E°_cell = E°_cathode - E°_anode.
Ensure that the units are consistent and the final E°_cell is expressed in volts (V).
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Textbook Question

Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. Ni2+(aq) + Mg(s) → Ni(s) + Mg2+(aq)

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Textbook Question

Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.

b. 2 H+(aq) + Fe(s) → H2(g) + Fe2+(aq)

c. 2 NO3–(aq) + 8 H+(aq) + 3 Cu(s) → 2 NO(g) + 4 H2O(l) + 3 Cu2+(aq)

Textbook Question

Calculate the standard cell potential for each of the electro- chemical cells in Problem 43.

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Textbook Question

Consider the voltaic cell:

d. Indicate the direction of anion and cation flow in the salt bridge

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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 notation. Write the overall balanced equation for the reaction and calculate E°cell. Sn(s) | Sn2+(aq) || NO(g) | NO3–(aq), H+(aq) | Pt(s)

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