a. Write the two balanced half-reactions involved and identify each in terms of (1) site of oxidation or reduction and(2) anode or cathode b. Calculate the net potential of the cell (the voltage), assuming standard conditions. c. Draw a neat fully labeled diagram of the galvanic cell using the half equations from part (a). Be sure to indicate the flow of electrons in the external circuit (through the wire) and the flow of all ions in the solution. Include a salt bridge.

Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 56QRT
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a. Write the two balanced half-reactions involved and identify each in terms of (1) site of oxidation or reduction and(2)
anode or cathode
b. Calculate the net potential of the cell (the voltage), assuming standard conditions.
c. Draw a neat fully labeled diagram of the galvanic cell using the half equations from part (a). Be sure to indicate the flow of electrons in the external circuit (through the wire) and the flow of all ions in the solution. Include a salt
bridge.
d. (i) Write the line notation of the cell. (ii) Describe in detail how this Galvanic cell is able to produce current.

Sn (s) + 2 Ag* → Sn* + 2 Ag (s)
Transcribed Image Text:Sn (s) + 2 Ag* → Sn* + 2 Ag (s)
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