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Byju's Answer
Standard XII
Chemistry
Nernst Equation
EMF of the ce...
Question
EMF of the cell:
C
u
/
C
u
2
+
(
0.01
M
)
|
|
C
u
2
+
(
0.001
M
)
|
C
u
is
(
E
0
C
u
2
+
/
C
u
=
+
0.34
V
)
A
0
V
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B
0.006
V
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C
0.03
V
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D
0.06
V
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Solution
The correct option is
C
0.03
V
E
∘
C
u
2
+
/
C
u
=
0.34
E
∘
C
u
/
C
u
2
+
=
−
0.34
E
o
c
e
l
l
=
E
o
r
e
d
−
E
o
o
x
∴
E
c
e
l
l
=
0.34
−
0.34
−
0.058
2
l
o
g
[
0.001
0.01
]
=
−
0.03
×
l
o
g
10
−
1
=
0.03
V
Option C is correct.
Suggest Corrections
3
Similar questions
Q.
Calculate the emf of the cell.
Z
n
|
Z
n
2
+
(
0.001
M
)
|
|
C
u
2
+
(
0.1
M
)
|
C
u
The standard potential of
C
u
/
C
u
2
+
half-cell is +0.34 and
Z
n
/
Z
n
2
+
is -0.76 V.
Q.
Calculate the emf of the cell
C
u
/
C
u
2
+
(
1
M
)
/
/
A
g
+
(
0.01
M
)
/
A
g
at
25
o
C. Given:
E
o
A
g
=
0.8
V,
E
o
C
u
=
0.34
V.
Q.
The electrode potentials for:
C
u
2
+
(
a
q
)
+
e
−
→
C
u
+
(
a
q
)
C
u
+
(
a
q
)
+
e
−
→
C
u
(
s
)
are + 0.15 V and 0.50 V respectively. The value of
E
0
c
u
2
/
C
u
will be :
Q.
The standard reduction potentials of
C
u
2
+
/
C
u
and
C
u
2
+
/
C
u
+
are
0.337
V
and
0.153
V
respectively. The standard electrode potential of
C
u
+
/
C
u
half-cell is:
Q.
The
E
⊖
f
o
r
C
u
2
+
/
C
u
⊕
,
C
u
⊕
/
C
u
,
C
u
2
+
/
C
u
,
are 0.15 V, 0.50 V, and 0.325 V, respectively. The redox cell showing redox reaction
2
C
u
+
,
→
C
u
2
+
+
C
u
is made.
E
⊖
of this cell reaction and
Δ
G
⊖
may be :
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