Page 900 - Chemistry--atom first
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890 Chapter 16 | Electrochemistry
7. Identify the species that undergoes oxidation, the species that undergoes reduction, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem.
8. Balance the following in basic solution:
(a)
(b)
(c)
(d)
9. Identify the species that was oxidized, the species that was reduced, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem.
10. Why is it not possible for hydroxide ion (OH−) to appear in either of the half-reactions or the overall equation when balancing oxidation-reduction reactions in acidic solution?
11. Why is it not possible for hydrogen ion (H+) to appear in either of the half-reactions or the overall equation when balancing oxidation-reduction reactions in basic solution?
12. Why must the charge balance in oxidation-reduction reactions? 16.2 Galvanic Cells
13.
(a)
(b)
(c)
(d)
14.
(a)
(b)
15. 16.
are (a)
(b)
(c)
(d)
17.
Write the following balanced reactions using cell notation. Use platinum as an inert electrode, if needed.
Given the following cell notations, determine the species oxidized, species reduced, and the oxidizing agent and reducing agent, without writing the balanced reactions.
For the cell notations in the previous problem, write the corresponding balanced reactions.
Balance the following reactions and write the reactions using cell notation. Ignore any inert electrodes, as they never part of the half-reactions.
Identify the species oxidized, species reduced, and the oxidizing agent and reducing agent for all the reactions in the previous problem.
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