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Byju's Answer
Standard XII
Chemistry
Redox Reactions and Couple
Half Reaction...
Question
Half Reaction
Eo
I.
M
g
→
M
g
2
+
+
2
e
−
2.37V
II.
M
n
→
M
n
2
+
+
2
e
−
1.03V
III.
H
2
→
2
H
+
+
2
e
−
0.00V
IV.
C
u
→
C
u
2
+
+
2
e
−
-0.16V
From the above experimental data which of the following represents a spontaneous process?
A
M
n
2
+
+
H
2
→
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B
M
g
+
M
n
2
+
→
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C
M
g
2
+
+
M
n
→
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D
C
u
+
2
H
+
→
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E
M
g
2
+
+
C
u
→
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Solution
The correct option is
D
M
g
+
M
n
2
+
→
E
0
A
=
(
0.00
−
1.03
)
=
−
1.03
V
E
0
B
=
(
2.37
−
1.03
)
=
1.34
V
E
0
C
=
(
1.03
−
2.37
)
=
−
1.34
V
E
0
D
=
(
−
0.16
−
0.00
)
=
−
0.16
V
E
0
E
=
(
−
0.16
−
2.37
)
=
−
2.53
V
Reaction is feasible if
E
0
is positive. Therefore, only reaction B is possible.
Suggest Corrections
0
Similar questions
Q.
Half Reaction
Eo
I.
M
g
→
M
g
2
+
+
2
e
−
2.37V
II.
M
n
→
M
n
2
+
+
2
e
−
1.03V
III.
H
2
→
2
H
+
+
2
e
−
0.00V
IV.
C
u
→
C
u
2
+
+
2
e
−
-0.16V
From the above experimental data what will be the standard reduction potential which represents spontaneous process?
Q.
Refer to the following experimental data.
Half Reaction
Eo
I.
M
g
→
M
g
2
+
+
2
e
−
2.37V
II.
M
n
→
M
n
2
+
+
2
e
−
1.03V
III.
H
2
→
2
H
+
+
2
e
−
0.00V
IV.
C
u
→
C
u
2
+
+
2
e
−
-0.16V
What will be the standard reduction potential for the reaction:
M
g
+
M
n
2
+
→
M
g
2
+
+
M
n
?
Q.
Refer to the following experimental data.
Half Reaction
E
o
I.
M
g
→
M
g
2
+
+
2
e
−
2.37V
II.
M
n
→
M
n
2
+
+
2
e
−
1.03V
III.
H
2
→
2
H
+
+
2
e
−
0.00V
IV.
C
u
→
C
u
2
+
+
2
e
−
-0.16V
Which of the following reactions is spontaneous?
Q.
Rank the following elements by increasing ease of oxidation with most easily oxidized LAST:
C
d
,
C
u
,
N
i
,
F
e
Standard Reduction Potentials at
25
∘
C
Half-Reaction
E
∘
(
V
)
F
2
+
2
e
−
→
2
F
−
2.87
A
g
2
+
e
−
→
A
g
+
1.99
C
o
3
+
+
e
−
→
C
o
2
+
1.82
H
2
O
2
+
2
H
+
+
2
e
−
→
2
H
2
O
1.78
M
n
O
−
4
+
4
H
+
+
3
e
−
→
M
n
O
2
+
2
H
2
O
1.68
2
e
−
+
2
H
+
+
I
O
−
4
→
I
O
−
3
+
H
2
O
1.60
M
n
O
−
4
+
8
H
+
+
5
e
−
→
M
n
2
+
+
4
H
2
O
1.51
A
u
3
+
+
3
e
−
→
A
u
1.50
C
l
2
+
2
e
−
→
2
C
l
−
1.36
O
2
+
4
H
+
+
4
e
−
→
2
H
2
O
1.23
M
n
O
2
+
4
H
+
+
2
e
−
→
M
n
2
+
+
2
H
2
O
1.21
B
r
2
+
2
e
−
→
2
B
r
−
1.09
N
O
−
3
+
4
H
+
+
3
e
−
→
N
O
+
2
H
2
O
0.96
C
l
O
2
+
e
−
→
C
l
O
2
0.954
2
H
g
2
+
+
2
e
−
→
H
g
2
+
2
0.91
A
g
+
+
e
−
→
A
g
0.80
H
g
2
+
2
+
2
e
−
→
2
H
g
0.80
F
e
3
+
+
e
−
→
F
e
2
+
0.77
O
2
+
2
H
+
+
2
e
−
→
H
2
O
2
0.68
M
n
O
−
4
+
e
−
→
M
n
O
2
−
4
0.56
I
2
+
2
e
−
→
2
I
−
0.54
C
u
+
+
e
−
→
C
u
0.52
O
2
+
2
H
2
O
+
4
e
−
→
4
O
H
−
0.40
C
u
2
+
+
2
e
−
→
C
u
0.34
A
g
C
l
+
e
−
→
A
g
+
C
l
−
0.22
C
u
2
+
+
e
−
→
C
u
+
0.16
2
H
+
+
2
e
−
→
H
2
0.00
F
e
3
+
+
3
e
−
→
F
e
−
0.036
P
b
2
+
+
2
e
−
→
P
b
−
0.13
N
i
2
+
+
2
e
−
→
N
i
−
0.23
C
d
2
+
+
2
e
−
→
C
d
−
0.40
F
e
2
+
+
2
e
−
→
F
e
−
0.44
C
r
3
+
+
e
−
→
C
r
2
+
−
0.50
C
r
3
+
+
3
e
−
→
C
r
−
0.73
Z
n
2
+
+
2
e
−
→
Z
n
−
0.76
2
H
2
O
+
2
e
−
→
H
2
+
2
O
H
−
−
0.83
M
n
2
+
+
2
e
−
→
M
n
−
1.18
A
l
3
+
+
3
e
−
→
A
l
−
1.66
H
2
+
2
e
−
→
2
H
−
−
2.23
M
g
2
+
+
2
e
−
→
M
g
−
2.37
N
a
+
+
e
−
→
N
a
−
2.71
C
a
2
+
+
2
e
−
→
C
a
−
2.76
B
a
2
+
+
2
e
−
→
B
a
−
2.90
K
+
+
e
−
→
K
−
2.92
L
i
+
+
e
−
→
L
i
−
3.05
Q.
Find the
△
G
∘
of a galvanic cell with
A
g
and
A
l
.
Standard Reduction Potentials at
25
∘
C
Half-Reaction
E
∘
(
V
)
F
2
+
2
e
−
→
2
F
−
2.87
A
g
2
+
e
−
→
A
g
+
1.99
C
o
3
+
+
e
−
→
C
o
2
+
1.82
H
2
O
2
+
2
H
+
+
2
e
−
→
2
H
2
O
1.78
M
n
O
−
4
+
4
H
+
+
3
e
−
→
M
n
O
2
+
2
H
2
O
1.68
2
e
−
+
2
H
+
+
I
O
−
4
→
I
O
−
3
+
H
2
O
1.60
M
n
O
−
4
+
8
H
+
+
5
e
−
→
M
n
2
+
+
4
H
2
O
1.51
A
u
3
+
+
3
e
−
→
A
u
1.50
C
l
2
+
2
e
−
→
2
C
l
−
1.36
O
2
+
4
H
+
+
4
e
−
→
2
H
2
O
1.23
M
n
O
2
+
4
H
+
+
2
e
−
→
M
n
2
+
+
2
H
2
O
1.21
B
r
2
+
2
e
−
→
2
B
r
−
1.09
N
O
−
3
+
4
H
+
+
3
e
−
→
N
O
+
2
H
2
O
0.96
C
l
O
2
+
e
−
→
C
l
O
2
0.954
2
H
g
2
+
+
2
e
−
→
H
g
2
+
2
0.91
A
g
+
+
e
−
→
A
g
0.80
H
g
2
+
2
+
2
e
−
→
2
H
g
0.80
F
e
3
+
+
e
−
→
F
e
2
+
0.77
O
2
+
2
H
+
+
2
e
−
→
H
2
O
2
0.68
M
n
O
−
4
+
e
−
→
M
n
O
2
−
4
0.56
I
2
+
2
e
−
→
2
I
−
0.54
C
u
+
+
e
−
→
C
u
0.52
O
2
+
2
H
2
O
+
4
e
−
→
4
O
H
−
0.40
C
u
2
+
+
2
e
−
→
C
u
0.34
A
g
C
l
+
e
−
→
A
g
+
C
l
−
0.22
C
u
2
+
+
e
−
→
C
u
+
0.16
2
H
+
+
2
e
−
→
H
2
0.00
F
e
3
+
+
3
e
−
→
F
e
−
0.036
P
b
2
+
+
2
e
−
→
P
b
−
0.13
N
i
2
+
+
2
e
−
→
N
i
−
0.23
C
d
2
+
+
2
e
−
→
C
d
−
0.40
F
e
2
+
+
2
e
−
→
F
e
−
0.44
C
r
3
+
+
e
−
→
C
r
2
+
−
0.50
C
r
3
+
+
3
e
−
→
C
r
−
0.73
Z
n
2
+
+
2
e
−
→
Z
n
−
0.76
2
H
2
O
+
2
e
−
→
H
2
+
2
O
H
−
−
0.83
M
n
2
+
+
2
e
−
→
M
n
−
1.18
A
l
3
+
+
3
e
−
→
A
l
−
1.66
H
2
+
2
e
−
→
2
H
−
−
2.23
M
g
2
+
+
2
e
−
→
M
g
−
2.37
N
a
+
+
e
−
→
N
a
−
2.71
C
a
2
+
+
2
e
−
→
C
a
−
2.76
B
a
2
+
+
2
e
−
→
B
a
−
2.90
K
+
+
e
−
→
K
−
2.92
L
i
+
+
e
−
→
L
i
−
3.05
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