. Consider the oxidation—reduction reaction Zn ( s ) + Pb 2+ ( a q ) → Zn 2 + ( a q ) + Pb ( s ) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?
Solution Summary: The author explains that oxidation and reduction can be identified by change in atom of an element, and if it decreases, it undergoes reduction.
Zn
(
s
)
+
Pb
2+
(
a
q
)
→
Zn
2
+
(
a
q
)
+
Pb
(
s
)
Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
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