5) In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ags) in the cathode half-cell. The standard potential of the half-reactions are as follows: Ag* (ag)+ e→ Ag(s) → Cu(s) E°red = +0.80 V Cu²+ (ад) +2 е > E°red = +0.34 V a) What is the standard potential of the cell, E°cell? b) Is the reaction spontaneous or non-spontaneous?

Question
5) In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ags) in the
cathode half-cell. The standard potential of the half-reactions are as follows:
Ag* (ag)+ e→ Ag(s)
→ Cu(s)
E°red = +0.80 V
Cu²+
(ад)
+2 е >
E°red = +0.34 V
a) What is the standard potential of the cell, E°cell?
b) Is the reaction spontaneous or non-spontaneous?
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Transcribed Image Text

5) In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ags) in the cathode half-cell. The standard potential of the half-reactions are as follows: Ag* (ag)+ e→ Ag(s) → Cu(s) E°red = +0.80 V Cu²+ (ад) +2 е > E°red = +0.34 V a) What is the standard potential of the cell, E°cell? b) Is the reaction spontaneous or non-spontaneous?

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