Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
Anode → oxidation
▪ oxidation half-reaction happens in the anode solution
▪ losing electrons → becoming more positive → anode dissolves away
Zn(s) → Zn2+ (aq)
Zn → anode → loses mass
Cathode → reduction
▪ reduction half-reaction happens in the anode solution
▪ gaining electrons → becoming more negative → solids is deposited in the surface
Cu2+(aq) → Cu(s)
Cu → cathode → gains mass
Describe the electrodes in this zinc-copper galvanic cell. Drag the appropriate items to their respective bins.
anode cathode gains mass loses mass
Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s)
Consider the following:
Zn2+ (aq) + 2e- → Zn(s), E° red = -0.763 V
Cu2+ (aq) + 2e- → Cu(s), E° red = +0.337 V
What is the standard potential, Ecell, for this galvanic cell? Use the given standard reduction potentials in your calculation as appropriate. Express your answer to three decimal places and include the appropriate units.
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