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Byju's Answer
Standard XII
Chemistry
Electrolytic Cell
An electroche...
Question
An electrochemical cell has two half cell reactions as,
A
2
+
+
2
e
−
⟶
A
;
E
o
=
0.34
V
X
⟶
X
2
+
+
2
e
−
;
E
o
=
2.37
V
Caclulate the
E
c
e
l
l
.
A
2.71V
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B
2.03V
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C
-2.71V
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D
-2.03V
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Solution
The correct option is
A
2.71V
Given reactions,
A
2
+
+
2
e
−
→
A
,
E
c
e
l
l
=
0.34
V
X
→
X
2
+
+
2
e
−
,
E
c
e
l
l
=
2.37
V
We know that,
E
c
e
l
l
=
E
c
a
t
h
o
d
e
−
E
a
n
o
d
e
At anode oxidation takes place and at cathode reduction takes place.
So,
E
c
e
l
l
=
2.37
−
(
−
0.34
)
=
2.71
V
Suggest Corrections
2
Similar questions
Q.
If for the half cell reactions
C
u
2
+
+
e
−
→
C
u
+
E
o
=
0.15
V
C
u
2
+
+
2
e
−
→
C
u
E
o
=
0.34
V
Calculate
E
o
of the half cell reaction
C
u
+
+
e
−
→
C
u
also predict whether
C
u
+
undergoes disproportionation or not.
Q.
In simple electrochemical cell, which is in its standard state, the
half cell reactions with their appropriate reduction potential are?
P
b
2
+
+
2
e
→
P
b
(
E
o
=
−
0.13
v
)
A
g
+
+
e
→
A
g
(
E
o
=
+
0.80
v
)
Q.
The standard reduction potentials EO, for the half reaction are as
Z
n
→
Z
n
+
+
+
2
e
−
,
E
0
=
0.76
V
C
u
→
C
u
+
+
+
2
e
−
,
E
0
=
0.34
V
The e.m.f. for the cell reaction,
Q.
The standard oxidation potentials,
E
o
, for the half cell reactions are as follows:
Z
n
→
Z
n
2
+
+
2
e
−
,
E
o
=
0.76
V
F
e
→
F
e
2
+
+
2
e
−
,
E
o
=
0.41
V
The EMF for the cell oxidation,
F
e
2
+
+
Z
n
→
Z
n
2
+
+
F
e
(Give your answer upto two decimal only)
Q.
The standard reduction potential
E
o
for the half reactions are as
Z
n
⟶
Z
n
2
+
+
2
e
−
;
E
o
=
+
0.76
V
F
e
⟶
F
e
2
+
+
2
e
−
;
E
o
=
+
0.41
V
The emf for cell reaction,
F
e
2
+
+
Z
n
⟶
Z
n
2
+
+
F
e
, is
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