9)
For Anode:


Zn2
/Zn
E

 = 
(
)
2+
o
Zn
/ Zn
E
 – RT
F
2  ln


2
1
Zn
aq





(2 10)
The cell potential, E(cell) = 


Cu2
/Cu
E

 – 


Zn2
/Zn
E

=
(
)
2+
o
Cu
/ Cu
E
 – RT
F
2  ln 
2+
1
Cu
(aq)




 – 
(
)
2+
o
Zn
/ Zn
E
 + RT
2F
 ln
2+
1
Zn
(aq)




=
(
)
2+
o
Cu
/ Cu
E
–
(
)
2+
o
Zn
/ Zn
E
– RT
F
2  




2+
2+
1
1
ln
 – ln
Cu
aq
Zn
aq








E(cell) = 
(
)
o
Ecell
 – RT
2F
 ln [
]
+
[
]
Zn2
2
Cu

(2 11)
It can be seen that E(cell) depends on the concentration of both Cu2+
and Zn2+ ions It increases with increase in the concentration of Cu2+
ions and decrease in the concentration of Zn2+ ions