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Byju's Answer
Standard XII
Chemistry
Characteristics of Equilibrium Constant
When 36.8g ...
Question
When 36.8g
N
2
O
4
is introduced into a 1 litre flask at 300 K. The following reaction occurs:
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
,
K
P
=
0.1642
atm.
Calculate the
K
C
of the equilibrium reaction.
Open in App
Solution
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
;
K
p
=
0.1642
a
t
m
K
P
=
K
C
(
R
T
)
Δ
n
Δ
n
=
2
−
1
=
1
,
R
=
0.0820
L
m
o
l
−
1
k
−
1
,
T
=
300
K
⇒
0.1642
=
K
C
(
0.082
×
300
)
1
⇒
K
C
=
0.1642
24.6
=
0.00667
=
6.67
×
10
−
3
m
o
l
d
m
−
3
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Similar questions
Q.
When 36.8g
N
2
O
4
(
g
)
is introduced into a 1.0-litre flask at
27
∘
C
. The following equilibrium reaction occurs:
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
;
K
p
=
0.1642
a
t
m
. Calculate
K
c
of the equilibrium reaction.
Q.
When
36.6
g
N
2
O
4
(
g
)
is introduced into a
1.0
−
l
i
t
r
e
flask at
27
∘
C
. The following equilibrium reaction occurs:
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
;
K
p
=
0.1642
a
t
m
.
(a) Calculate
K
c
of the equilibrium reaction?
(b) What are the number of moles of
N
2
O
4
and
N
O
2
at equilibrium?
(c) What is the total gas pressure in the flask at equilibrium?
(d) What is the percent dissociation of
N
2
O
4
?
Q.
9.2
g
r
a
m
s
of
N
2
O
4
(
g
)
is taken in a closed one-litre vessel and heated till the following equilibrium is reached.
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
At equilibrium,
50
%
N
2
O
4
(
g
)
is dissociated. What is the equilibrium constant? (in mol litre
−
1
)
[Molecular weight of
N
2
O
4
=
92
]
Q.
At the equilibrium of the reaction,
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
, the observed molar mass of
N
2
O
4
is
77.70
g
. The percentage dissociation of
N
2
O
4
is:
Q.
For the reaction in equilibrium,
N
2
O
4
(
g
)
⇌
2
N
O
2
(
g
)
The concentrations of
N
2
O
4
and
N
O
2
at equilibrium are
4.8
×
10
−
2
and
1.2
×
10
−
2
m
o
l
L
−
1
respectively. The value of
K
c
for this reaction is:
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