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Byju's Answer
Standard XII
Chemistry
Characteristics of Equilibrium Constant
When 1 mole...
Question
When
1
m
o
l
e
H
2
O
(
g
)
and
1
m
o
l
e
C
O
(
g
)
are heated at
1000
∘
C
in a closed vessel of
5
l
i
t
r
e
, it was found that
40
%
of
H
2
O
react at equilibrium according to
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
. Find
K
C
of the reaction.
Open in App
Solution
The given reaction is :-
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
Initial moles :
1
1
0
0
At eqm :
(
1
−
α
)
(
1
−
α
)
α
α
(let)
Now, given that, at equilibrium,
40
% of
H
2
O
has reacted
⇒
α
=
0.4
∴
At eqm, no. of moles of
H
2
O
=
0.6
No. of moles of
H
2
=
4
No. of moles of
C
O
2
=
0.4
So,
K
C
=
[
H
2
]
[
C
O
2
]
[
H
2
O
]
[
C
O
]
=
0.4
×
0.4
0.6
×
0.6
=
4
9
=
0.44
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Similar questions
Q.
When
1
mole
H
2
O
(
g
)
and
1
mole
C
O
(
g
)
are heated at
1000
∘
C
in a closed vessel of
5
litre, it will found that
40
% of
H
2
O
react at equilibrium according to
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
.
Q.
1
mole of
H
2
O
and
1
mole of
C
O
are heated in a
10
litre vessel at
1259
K
.
40
%
H
2
O
reacts with
C
O
according to the following equations,
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
;
Calculate equilibrium constant for the reaction.
Q.
O
n
e
m
o
l
e
of
H
2
O
and
o
n
e
m
o
l
e
of
C
O
were heated in a
10
L
closed vessel at
1260
K
. At equilibrium,
40
% of water was found to react in the equation,
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
Calculate the equilibrium constant of the reaction.
Q.
One mole of
H
2
O
and one mole of CO are taken in 10L vessel and heated to 725 K. At equilibrium 40% of water (by mass) reacts with CO according to the equation,
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
What is the value of equilibrium constant
(
K
c
)
for the reaction.
Q.
One mole of
H
2
O
and one mole of CO are taken in 10 L vessel and heated to 725 K. At equilibrium 40% of water reacts with CO according to the equation,
H
2
O
(
g
)
+
C
O
(
g
)
⇌
H
2
(
g
)
+
C
O
2
(
g
)
. What is the value of equilibrium constant
(
K
c
)
for the reaction?
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