Copper metal and zinc metal will both reduce Ag+ ions under standard state conditions. Which metal when used as an electrode in a galvanic cell will have the larger Eºcell? Show your work. (Hint: Write the two possible chemical reactions.) Standard Reduction Potentials: Ag+ (aq) + e¯ ⇒ Ag(s) Cu²+ (aq) + 2e Cu(s) ⇒ Zn²+ (aq) + 2e¯ ⇒ Zn(s) E E E cell - substance reduced - substance oxidized A +0.80 +0.34 -0.76

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Copper metal and zinc metal will both reduce Ag+ ions under standard
state conditions. Which metal when used as an electrode in a galvanic
cell will have the larger Eºcell? Show your work. (Hint: Write the two
possible chemical reactions.)
Standard Reduction Potentials:
Ag+ (aq) + e¯ = Ag(s)
Cu²+ (aq) +2e=Cu(s)
Zn²+ (aq) + 2e¯ ⇒ Zn(s)
-E
E
cell
= E
substance reduced
substance oxidized
L
+0.80
+0.34
-0.76
Transcribed Image Text:Copper metal and zinc metal will both reduce Ag+ ions under standard state conditions. Which metal when used as an electrode in a galvanic cell will have the larger Eºcell? Show your work. (Hint: Write the two possible chemical reactions.) Standard Reduction Potentials: Ag+ (aq) + e¯ = Ag(s) Cu²+ (aq) +2e=Cu(s) Zn²+ (aq) + 2e¯ ⇒ Zn(s) -E E cell = E substance reduced substance oxidized L +0.80 +0.34 -0.76
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