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Byju's Answer
Standard XII
Chemistry
Nernst Equation
E0Zn2+/Zn=-0....
Question
E
0
Z
n
2
+
/
Z
n
=
−
0.76
V
The EMF of the cell
Z
n
/
Z
n
2
+
(
1
M
)
|
|
H
C
l
(
p
H
=
2
)
|
H
2
(
1
a
t
m
)
,
P
t
is :
:
A
0.878
V
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B
0.642
V
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C
0.875
V
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D
0.700
V
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Solution
The correct option is
B
0.642
V
Given
−
l
o
g
[
H
+
]
=
2
∴
[
H
]
+
=
10
−
2
2
e
−
+
Z
n
2
+
→
Z
n
E
∘
=
−
0.76
Z
n
+
2
H
+
→
Z
n
2
+
+
H
2
∴
E
c
e
l
l
=
−
(
−
0.76
)
−
0.059
2
l
o
g
[
Z
n
2
+
]
[
H
+
]
2
=
0.76
−
0.059
2
×
2
p
H
=
0.76
−
0.059
2
×
2
×
2
=
0.642
V
Option B is correct.
Suggest Corrections
0
Similar questions
Q.
Reduction potential for the following half/cell reaction are
Z
n
→
Z
n
2
+
+
2
e
−
(
E
0
(
Z
n
2
+
/
Z
n
)
=
−
0.76
V
)
F
e
→
F
e
2
+
+
2
e
−
E
0
=
0.41
V
The EMF for the cell reaction
F
e
2
+
+
Z
n
→
Z
n
2
+
+
F
e
will
Q.
E
o
for the half cell
Z
n
2
+
|
Z
n
is
−
0.76
e.m.f. of the cell
Z
n
∣
∣
Z
n
2
+
(
1
M
)
∣
∣
∣
∣
2
H
+
(
1
M
)
∣
∣
H
2
(
1
a
t
m
)
:
Q.
The EMF of a cell :
Z
n
+
2
H
+
→
Z
n
2
+
(
0.1
M
)
+
H
2
(
1
a
t
m
)
is
0.28
V at
25
∘
C
. Calculate pH of the solution at the hydrogen gas electrode.
Given that :
E
⊖
(
Z
n
2
+
|
Z
n
)
=
−
0.76
V
.
Q.
Z
n
(
s
)
/
Z
n
2
+
(
a
q
)
∥
C
u
2
+
(
a
q
)
/
C
u
(
s
)
E
0
Z
n
2
+
/
Z
n
=
−
0.76V,
E
0
C
u
2
+
/
C
u
=
+
0.34V.
Calculate
E
0
c
e
l
l
and equilibrium constant
K
.
Q.
Calculate
E
∘
values of following reactions:
C
u
(
s
)
+
Z
n
2
+
(
a
q
)
→
Z
n
(
s
)
+
C
u
2
+
(
a
q
)
[Given:
E
0
C
u
2
+
/
C
u
=
0.34
V
,
E
0
Z
n
2
+
/
Z
n
=
−
0.76
V
]
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