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Byju's Answer
Standard XII
Chemistry
Introduction to Oxidation and Reduction
The reaction ...
Question
The reaction given below is interpreted as:
H
2
S
(
g
)
+
C
l
2
(
g
)
→
2
H
C
l
(
g
)
+
S
(
s
)
A
H
2
S
is getting oxidized and
C
l
2
is getting reduced
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B
H
2
S
is getting reduced and
C
l
2
is getting oxidized
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C
Only
H
2
S
is oxidized
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D
Both
H
2
S
and
C
l
2
are reduced
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Solution
The correct option is
A
H
2
S
is getting oxidized and
C
l
2
is getting reduced
H
2
S
(
g
)
+
C
l
2
(
g
)
⟶
2
H
C
l
(
g
)
+
S
(
s
)
Here, oxidation state of
S
changes from
−
2
to
0
.
Hence, it is getting oxidized.
Here, the oxidation state of
C
l
changes from
0
to
−
1
Hence, it is getting reduced.
Therefore, option
A
is the correct answer.
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0
Similar questions
Q.
In the reaction, H
2
S + Cl
2
→ 2HCl + S; hydrogen sulphide is:
Q.
2
H
2
S
+
S
O
2
→
3
S
+
2
H
2
O
In the above reaction:
(a)
H
2
S
gets oxidized.
(b)
S
O
2
gets reduced.
(c)
H
2
S
gets reduced.
(d)
S
O
2
gets oxidized.
Q.
In the reaction given below, identify the specie undergoing oxidation and reduction
H
2
S
(
g
)
+
C
l
2
→
2
H
C
l
(
g
)
+
S
(
s
)
Q.
In the reaction
H
2
S
+
C
l
2
→
2
H
C
l
+
S
, the oxidizing agent is :
Q.
Consider the reaction :
C
l
2
(
a
q
)
+
H
2
S
(
a
q
)
→
S
(
s
)
+
2
H
+
(
a
q
)
+
2
C
l
−
(
a
q
)
The rate equation for this reaction is
=
k
[
C
l
2
]
[
H
2
S
]
Which of these mechanisms
i
s
/
a
r
e
consistent with this rate equation?
(A)
C
l
2
+
H
2
S
→
H
+
+
C
l
−
+
C
l
+
+
H
S
−
(slow)
C
l
+
+
H
S
−
→
H
+
+
C
l
−
+
S
(fast)
(B)
H
2
S
⇔
H
+
+
H
S
−
(fast equilibrium)
C
l
2
+
H
S
−
→
2
C
l
−
+
H
+
+
S
(slow)
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