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Byju's Answer
Standard XII
Chemistry
SHE
The potential...
Question
The potential of the cell containing two hydrogen electrodes as represented below, is:
P
t
,
H
2
(
g
)
|
H
+
(
10
−
6
M
)
|
|
H
+
(
10
−
4
M
)
|
H
2
(
g
)
,
P
t
at
298
K
A
−
0.118
V
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B
−
0.0591
V
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C
0.118
V
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D
0.0591
V
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Solution
The correct option is
C
0.118
V
At cathode:
H
+
c
+
e
−
⟶
1
/
2
H
2
E
o
=
0
V
At anode:
1
/
2
H
2
⟶
H
+
a
+
e
−
E
o
=
0
V
_____________________
Cell reaction
H
+
c
⟶
H
+
a
E
o
c
e
l
l
=
0
For concentration
E
o
c
e
l
l
is
0
, as both the compartment have same half cell.
Using Nernst Equation
[
H
+
]
a
=
concentration of
H
+
at anode;
[
H
+
]
c
=
concentration of
H
+
at cathode
⇒
E
c
e
l
l
=
E
o
c
e
l
l
−
0.0591
1
log
[
H
+
]
a
[
H
+
]
c
⇒
E
c
e
l
l
=
−
0.0591
log
[
10
−
6
]
[
10
−
4
]
⇒
E
c
e
l
l
=
−
0.0591
log
10
−
2
⇒
E
c
e
l
l
=
2
×
0.0591
=
0.1182
V
Suggest Corrections
0
Similar questions
Q.
What is the potential of the cell containing two hydrogen electrodes as represented below?
P
t
;
1
/
2
H
2
(
g
)
|
H
+
(
10
−
8
M
)
|
|
H
+
(
0.001
M
)
|
1
/
2
H
2
(
g
)
P
t
1 atm 1 atm
Q.
Standard hydrogen electrode is represented as
P
t
(
s
)
,
H
+
(
a
q
)
|
H
2
(
g
)
.
Q.
What is the potential of the cell containing two hydrogen electrodes as represented below ?
p
t
;
1
2
H
2
(
g
)
|
H
2
O
|
|
H
⊕
(
0.001
M
)
|
1
/
2
H
2
(
g
)
P
t
Q.
The cell
P
t
,
H
2
(
g
)
(
1
atm
)
/
H
+
,
p
H
=
x
|
|
Normal calomel electrode has emf of
0.67
V
at
25
∘
C
. The oxidation potential of calomel electrode on H scale is
−
0.28
V
, then
p
H
of solution will be
(Given :
2.303
R
T
F
=
0.0591
V
)
Q.
In the cell
P
t
(
s
)
,
H
2
(
g
)
|
1
b
a
r
H
C
l
(
a
q
)
|
A
g
(
s
)
|
P
t
(
s
)
the cell potential is
0.92
when
10
−
6
molal
H
C
l
solution is used. The standard electrode potential of
(
A
g
C
l
/
A
g
,
C
l
−
)
electrode is:
[Given:
2.303
R
T
F
=
0.06
V
at
298
K
]
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