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Byju's Answer
Standard XII
Chemistry
Nernst Equation
Zn | Zn2+ aq ...
Question
Z
n
|
Z
n
2
+
(
a
q
)
|
|
C
u
2
+
(
a
q
)
|
C
u
.
E
o
for
C
u
and
Z
n
are
0.35
and
−
0.76
respectively:
Find EMF of cell (nearest integer) if
Z
n
2
+
and
C
u
2
+
are 1 M each.
Open in App
Solution
E
0
c
e
l
l
=
E
0
C
u
2
+
|
C
u
−
E
0
Z
n
2
+
|
Z
n
E
0
c
e
l
l
=
0.35
V
−
(
−
0.76
V
)
E
0
c
e
l
l
=
1.11
V
Now,
E
c
e
l
l
=
E
0
c
e
l
l
−
0.0591
n
l
o
g
[
Z
n
2
+
]
[
C
u
2
+
]
E
c
e
l
l
=
1.11
V
−
0.0591
2
l
o
g
1
1
E
c
e
l
l
=
1.11
V
−
0
E
c
e
l
l
=
1.11
V
Suggest Corrections
0
Similar questions
Q.
The values for cell is
Z
n
|
Z
n
2
+
(
a
q
)
|
|
C
u
2
+
(
a
q
)
|
C
u
E
o
for Cu and Zn are
0.35
and
−
0.76
respectively:
then what will be the cell reaction?
Q.
Consider the cell:
Z
n
|
Z
n
2
+
(
a
q
)
(
1.0
M
)
|
|
C
u
2
+
(
a
q
)
(
1.0
M
)
|
|
C
u
The standard reduction potential are 0.350 V for
C
u
2
+
(
a
q
)
+
2
e
−
→
C
u
and -0.763 V for
Z
n
2
+
(
a
q
)
+
2
e
−
→
Z
n
.
The EMF (in V) of the cell is
( write your answer as nearest integer) :
Q.
Consider the cell,
Z
n
|
Z
n
2
+
(
a
q
)
(
1.0
M
)
|
|
C
u
2
+
(
a
q
)
(
1.0
M
)
|
C
u
The standard reduction potentials are
+
0.35
V
for
2
e
−
+
C
u
2
+
(
a
q
)
→
C
u
2
+
(
a
q
)
(
1.0
M
)
|
C
u
The standard reduction potentials are
+
0.35
V
for
2
e
−
+
C
u
2
+
(
a
q
)
→
C
u
and
−
0.763
V
for
2
e
−
+
Z
n
2
+
(
a
q
)
→
Z
n
Calculate the emf of the cell and tell whether the cell reaction spontaneous or not ?
Q.
Consider the cell:
Z
n
|
Z
n
2
+
(
a
q
)
(
1.0
M
)
|
|
C
u
2
+
(
a
q
)
(
1.0
M
)
|
|
C
u
The standard reduction potential are
0.350
V for
C
u
2
+
(
a
q
)
+
2
e
−
→
C
u
and
−
0.763
V for
Z
n
2
+
(
a
q
)
+
2
e
−
→
Z
n
The cell reaction is:
Q.
For cell reaction,
Z
n
+
C
u
2
+
→
Z
n
2
+
+
C
u
,
cell representation is