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Byju's Answer
Standard XII
Chemistry
Nernst Equation
Consider the ...
Question
Consider the following cell reaction:
2
F
e
(
s
)
+
O
2
(
g
)
+
4
H
+
(
a
q
)
→
2
F
e
2
+
(
a
q
)
+
2
H
2
O
(
l
)
;
E
o
=
1.67
V
At
[
F
e
2
+
]
=
10
−
3
M
,
P
O
2
=
0.1
atm and
p
H
=
3
, the cell potential at 25
o
C
is:
A
1.47
V
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B
1.77
V
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C
1.87
V
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D
1.57
V
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Solution
The correct option is
D
1.57
V
p
H
=
3
⇒
[
H
+
]
=
10
−
3
M
Now,
E
c
e
l
l
=
E
o
−
0.059
4
l
o
g
[
F
e
2
+
]
2
[
H
+
]
4
P
O
2
=
1.67
−
0.059
4
l
o
g
(
10
−
3
)
2
(
10
−
3
)
4
×
0.1
=
1.67
−
0.059
4
l
o
g
10
7
=
1.67
−
0.059
4
×
7
=
1.67
−
0.105
=
1.565
=
1.57
V
.
Option D is correct.
Suggest Corrections
0
Similar questions
Q.
Consider the following cell reaction:
2
F
e
(
s
)
+
O
2
(
g
)
+
4
H
+
(
a
q
)
→
2
F
e
2
+
(
a
q
)
+
2
H
2
O
(
l
)
E
−
=
1.67
V
At
[
F
e
2
+
]
=
10
−
3
M
,
p
(
O
2
)
=
0.1
atm and
p
H
=
3
.
The cell potential at
25
0
C is:
Q.
Consider the following cell reaction:
2
F
e
(
s
)
+
O
2
(
g
)
+
4
H
+
(
a
q
)
→
2
F
e
2
+
(
a
q
)
+
2
H
2
O
(
l
)
;
E
∘
=
1.67
V
At
[
F
e
2
+
]
=
10
−
3
M
,
P
(
O
2
)
=
0.1
a
t
m
and pH = 3, the cell potential at
25
∘
C
is
(given:
2.303
R
T
F
=
0.0591
)
Q.
Consider the following cell reaction:
2
F
e
(
s
)
+
O
2
(
g
)
+
4
H
+
(
a
q
)
→
2
F
e
2
+
(
a
q
)
+
2
H
2
O
(
l
)
;
E
∘
=
1.67
V
At
[
F
e
2
+
]
=
10
−
3
M
,
P
(
O
2
)
=
0.1
a
t
m
and pH = 3, the cell potential at
25
∘
C
is
(given:
2.303
R
T
F
=
0.0591
)
Q.
What is the cell potential (standard emf,
E
o
) for the reaction below ?
[
E
o
(
F
e
2
+
(
a
q
)
/
F
e
)
=
0.44
V
and
E
o
(
O
2
(
g
)
/
H
2
O
/
O
H
−
)
=
+
0.4
V
]
2
F
e
(
s
)
+
O
2
(
g
)
+
2
H
2
O
(
l
)
⇋
2
F
e
2
+
(
a
q
)
+
4
O
H
−
(
a
q
)
Q.
Calculate the reduction potential for the given half cells at
25
o
C
.
P
t
(
s
)
|
F
e
2
+
(
a
q
,
0.1
M
)
,
F
e
3
+
(
a
q
,
0.01
M
)
;
E
0
F
e
3
+
/
F
e
2
+
=
+
0.77
V
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