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Byju's Answer
Standard XII
Chemistry
Nernst Equation
Calculate E...
Question
Calculate
E
o
C
e
l
l
value of the following reactions:
Z
n
(
s
)
+
C
u
2
+
(
a
q
)
→
Z
n
2
+
(
a
q
)
+
C
u
(
s
)
[Given:
E
∘
C
u
2
+
/
C
u
=
0.34
V
,
E
∘
Z
n
2
+
/
Z
n
=
−
0.76
V
]
A
−
0.42
V
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B
0.46
V
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C
−
0.46
V
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D
1.1
V
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Solution
The correct option is
C
1.1
V
Given:
E
∘
C
u
2
+
/
C
u
=
0.34
V
,
E
∘
Z
n
2
+
/
Z
n
=
−
0.76
V
C
u
2
+
(
a
q
)
+
2
e
−
→
C
u
(
s
)
;
E
∘
r
e
d
n
=
+
0.34
V
Z
n
2
+
(
a
q
)
+
2
e
−
→
Z
n
(
s
)
;
E
∘
r
e
d
n
=
−
0.76
V
a
n
d
E
o
o
x
d
n
=
+
0.76
V
In the given reaction,
C
u
is reduced and
Z
n
is oxidized.
Z
n
(
s
)
+
C
u
2
+
(
a
q
)
⟶
Z
n
2
+
(
a
q
)
+
C
u
(
s
)
E
o
=
E
o
o
x
i
d
a
t
i
o
n
+
E
o
r
e
d
u
c
t
i
o
n
=
0.76
+
0.34
=
1.1
V
Hence, option (D) is correct.
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Similar questions
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
]
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.
At
298
K
, given that:
C
u
(
s
)
|
C
u
2
+
(
1.0
M
)
|
|
A
g
+
(
1.0
M
)
|
A
g
(
s
)
E
o
c
e
l
l
=
0.46
V
Z
n
(
s
)
|
Z
n
2
+
(
1.0
M
)
|
|
C
u
2
+
(
1.0
M
)
|
C
u
(
s
)
E
o
c
e
l
l
=
1.10
V
Then, the
E
c
e
l
l
for the following reaction at
298
K
will be:
Z
n
(
s
)
|
Z
n
2
+
(
0.1
M
)
|
|
A
g
+
(
1.
0
M
)
|
A
g
(
s
)
Q.
E
∘
for the cell,
Zn(s)|Zn
2
+
(
aq
)
|
|
Cu
2
+
(aq)|Cu(s)
is
1.10
V at
25
∘
C
. The equilibrium constant for the reaction,
Zn(s)
+
Cu
2
+
(aq)
→
Cu(s)
+
Zn
2
+
(aq)
is
1.94
×
10
x
. The value of
x
is
Q.
E
∘
for the cell is
Z
n
|
Z
n
2
+
(
a
q
)
|
|
C
u
2
+
(
a
q
)
|
C
u
at
25
∘
C
, the equilibrium constant for the reaction
Z
n
+
C
u
2
+
(
a
q
)
⇌
C
u
+
Z
n
2
+
(
a
q
)
is of the order of
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