(2 11) to the base 10 and
substituting the values of R, F and T = 298 K, it reduces to
E(cell) = 
(
)
o
Ecell
 – 
0 059
2
2
2 [
]
[
]
log Zn
Cu
+
+
(2 12)
We should use the same number of electrons (n) for both the
electrodes and thus for the following cell
Ni(s)ú Ni2+(aq) úú Ag+(aq)ú Ag
The cell reaction is Ni(s) + 2Ag+(aq) ® Ni2+(aq) + 2Ag(s)
The Nernst equation can be written as
E(cell) = 
(
)
o
Ecell
 – RT
F
2  ln [Ni
]
[Ag ]
2+
2
+
and for a general electrochemical reaction of the type:
a A + bB 
ne–
 cC + dD
Nernst equation can be written as:
E(cell) = 
(
)
o
Ecell
 – 
RT
nF 1nQ
= 
(
)
o
Ecell
 – 
RT
nF  ln
[C] [D]
[A] [B]
c
d
a
b
(2