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Byju's Answer
Standard XII
Chemistry
Oxidation Number Method
Balance the f...
Question
Balance the following redox reaction in basic medium:
M
n
2
+
+
C
l
O
−
3
⟶
M
n
O
2
+
C
l
O
2
A
M
n
2
+
+
2
C
l
O
−
3
⟶
M
n
O
2
+
2
C
l
O
2
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B
M
n
2
+
+
3
C
l
O
−
3
⟶
M
n
O
2
+
3
C
l
O
2
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C
M
n
2
+
+
4
C
l
O
−
3
⟶
M
n
O
2
+
4
C
l
O
2
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D
None of these
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Solution
The correct option is
A
M
n
2
+
+
2
C
l
O
−
3
⟶
M
n
O
2
+
2
C
l
O
2
The unbalanced redox equation is as follows:
M
n
2
+
+
C
l
O
−
3
⟶
M
n
O
2
+
C
l
O
2
All atoms other than H and O are balanced.
The oxidation number of Mn changes from 2 to 4. The change in the oxidation number is 2.
The oxidation number of Cl changes from 5 to 4. The change in he oxidation number is 1.
To balance the increase in the oxidation number with decrease in the oxidation number multiply
C
l
O
−
3
and
C
l
O
2
with 2.
M
n
2
+
+
2
C
l
O
−
3
⟶
M
n
O
2
+
2
C
l
O
2
This is the balanced chemical equation.
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0
Similar questions
Q.
Write balanced redox reactions of the following.
H
2
O
2
(
a
q
)
oxidises
M
n
2
+
(
a
q
)
to
M
n
O
2
in basic medium.
Q.
The following two redox reactions are given:
i)
M
n
O
−
4
+
8
H
+
+
5
e
−
→
M
n
2
+
+
4
H
2
O
;
E
o
=
X
1
V
ii)
M
n
O
2
+
4
H
+
+
2
e
−
→
M
n
2
+
+
2
H
2
O
;
E
o
=
X
2
V
Find
E
o
for the following reaction.
M
n
O
−
4
+
4
H
+
+
3
e
−
→
M
n
O
2
+
2
H
2
O
Q.
Calculate the value of
E
∘
M
n
O
−
4
|
M
n
O
2
.
M
n
O
−
4
+
8
H
+
+
5
e
−
→
M
n
2
+
+
4
H
2
O
;
E
∘
=
1.51
V
M
n
O
2
+
4
H
+
+
2
e
−
→
M
n
2
+
+
2
H
2
O
;
E
∘
=
1.23
V
Q.
E
∘
for the half cells :
M
n
O
2
+
4
H
+
+
2
e
−
→
M
n
2
+
+
2
H
2
O
i
s
1.23
V
F
e
3
+
+
e
−
→
F
e
2
+
i
s
0.77
V
Which of the following statements is true?
Q.
Given the standard potential of the following at
25
∘
C
.
M
n
O
2
→
M
n
3
+
;
E
⊖
=
0.95
V
M
n
3
+
→
M
n
2
+
;
E
⊖
=
1.51
V
The standard potential of
M
n
O
2
→
M
n
2
+
is:
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