1
Electrochemistry
L.E.O.
G.E.R.
Cu Cu2+ + 2e
Fe3+ + e Fe2+
Al + CuCl2 AlCl3 + Cu
FeCl3 + H2S FeCl2 + S + HCl
Cr2O72(aq)+ Cl(aq) Cr3+(aq)+ Cl2(g) (acidic)
MnO4− + SO32− → Mn2+ + SO42− (acidic)
Cr + ClO4− → CrO2− + ClO3− (basic)
H2O H+
"OTHER" O H e OH
2
Standard Reduction Potentials
Galvanic Cell
Why 1.10 V? Zn(s)|Zn2+(aq) ||Cu2+(aq) |Cu(s)anode cathode
Ni Al
Ni2+ Al3+
Fe Ag
Fe Au
Au1+Fe3+
Ni Cu
Cu2+Ni2+
Fe3+ Ag+
3
F = 96,485
ΔGo = n F Eo
Spontaneity
Cmol
Eo = +Eo =
# of e stransferred
4
The Nerst Equation
= 0.0592n log Q
@ 25oC
EoEcell
Q = K at equilibrium
Ecell = 0therefore
MnAl