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Standard XII
Chemistry
Electrolysis and Electrolytes
Standard redu...
Question
Standard reduction potentials of the half reactions are given below:
F
2
(
g
)
+
2
e
−
→
2
F
−
(
a
q
)
;
E
o
=
+
2.85
V
C
l
2
(
g
)
+
2
e
−
→
2
C
l
−
(
a
q
)
;
E
o
=
+
1.36
V
B
r
2
(
l
)
+
2
e
−
→
2
B
r
−
(
a
q
)
;
E
o
=
+
1.06
V
I
2
(
g
)
+
e
−
→
2
I
−
(
a
q
)
;
E
o
=
+
0.53
V
The strongest oxidising and reducing agents respectively are:
A
B
r
2
and
C
l
−
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B
C
l
2
and
B
r
−
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C
C
l
2
and
I
2
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D
F
2
and
I
−
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Solution
The correct option is
D
F
2
and
I
−
Fluorine is the strongest reducing agent as it has the highest value of standard reduction potential.
Iodide ion is the strongest reducing agent as it has the lowest value of the standard reduction potential.
As the value of the standard reduction potential decreases, the oxidizing power decreases and the reducing power increases.
Suggest Corrections
1
Similar questions
Q.
Standard reduction potentials of the half-reactions are given below:
F
2
(
g
)
+
2
e
−
→
2
F
−
(
a
q
)
:
E
0
=
+
2.85
V
C
l
2
(
g
)
+
2
e
−
→
2
C
l
−
(
a
q
)
:
E
0
=
+
1.36
V
B
r
2
(
l
)
+
e
−
→
2
B
r
−
(
a
q
)
:
E
0
=
+
1.06
V
I
2
(
g
)
+
e
−
→
2
I
−
(
a
q
)
:
E
0
=
+
0.53
V
The strongest oxidizing and reducing agent among the given reactions are ____________ respectively.
Q.
Standard reduction potentials of the half reactions are given below
F
2
(
g
)
+
2
e
−
→
2
F
−
(
a
q
)
;
E
0
=
+
2.85
V
C
l
2
(
g
)
+
2
e
−
→
2
C
l
−
(
a
q
)
;
E
0
=
+
1.36
V
B
r
2
(
l
)
+
2
e
−
→
2
B
r
−
(
a
q
)
;
E
0
=
+
1.06
V
I
2
(
s
)
+
2
e
−
→
2
I
−
(
a
q
)
;
E
0
=
+
0.53
V
The strongest oxidising and reducing agents respectively are:
Q.
The standard reduction potentials at 298K for the following half cell reaction are given below:
Z
n
2
+
(
a
q
)
+
2
e
−
⇌
Z
n
(
s
)
;
E
o
=
−
0.762
V
C
r
3
+
(
a
q
)
+
3
e
−
⇌
C
r
(
s
)
;
E
o
=
+
0.762
V
2
H
+
(
a
q
)
+
2
e
−
⇌
H
2
(
g
)
;
E
o
=
+
0.00
V
F
e
3
+
(
a
q
)
+
e
−
⇌
F
e
2
+
(
a
q
)
;
E
o
=
+
0.770
V
Based on the above reactions, select the strongest reducing agent?
Q.
Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titrations. Some half cell reactions and their standard potentials are given below:
M
n
O
−
4
(
a
q
.
)
+
8
H
+
(
a
q
.
)
+
5
e
−
→
M
n
2
+
(
a
q
.
)
+
4
H
2
O
(
l
)
;
E
o
=
1.51
V
C
r
2
O
2
−
7
(
a
q
.
)
+
14
H
+
(
a
q
.
)
+
6
e
−
→
2
C
r
3
+
(
a
q
.
)
+
7
H
2
O
(
l
)
;
E
o
=
1.38
V
F
e
3
+
(
a
q
.
)
+
e
−
→
F
e
2
+
(
a
q
.
)
;
E
o
=
0.77
V
C
l
2
(
g
)
+
2
e
−
→
2
C
l
−
(
a
q
.
)
;
E
o
=
1.40
V
Identify the only incorrect statement regarding the quantitative estimation of aqueous
F
e
(
N
O
3
)
2
.
Q.
Electrode potential data are given
F
e
3
+
(
a
q
)
+
e
−
→
F
e
2
+
(
a
q
)
;
E
o
=
+
0.77
V
A
l
3
+
(
a
q
)
+
3
e
−
→
A
l
s
;
E
o
=
−
1.66
V
B
r
2
(
a
q
)
+
2
e
−
→
2
B
r
−
(
a
q
)
;
E
o
=
+
1.66
V
Based on the given data which statement(s) is/are incorrect?
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