[Cu2+] = 1.6x10-18 M
Cu2+ (aq) + 2 e- → Cu (s) E° = 0.34 V ↓ E → oxidation → anode
Ag+ (aq) + e- → Ag (s) E° = 0.80 V ↑ E → reduction → cathode
E°cell = 0.46 V
Cu (s) → Cu2+ (aq) + 2 e-
[Ag+ (aq) + e- → Ag (s)] x2
2 Ag+ (aq) + Cu (s) → Cu2+ (aq) + 2 Ag (s)
n = 2
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag +] = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 M NH3 that is also 0.010 M in Cu(NH 3)4 2+, what is the cell potential at 25°C?
Cu2+(aq) + 4NH3 (aq) ⇌ Cu(NH 3)4 2+(aq) K = 1.0 X 10 13
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