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Byju's Answer
Standard XII
Chemistry
Gibbs Free Energy & Spontaneity
The INCORRECT...
Question
The INCORRECT match in the following is :
A
Δ
G
0
<
0
,
K
<
1
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B
Δ
G
0
<
0
,
K
=
1
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C
Δ
G
0
>
0
,
K
<
1
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D
Δ
G
0
<
0
,
K
>
1
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Solution
The correct option is
A
Δ
G
0
<
0
,
K
<
1
We know,
Δ
G
=
Δ
G
0
+
R
T
l
n
K
At equilibrium,
Δ
G
=
Δ
G
0
+
R
T
l
n
K
=
0
⇒
Δ
G
0
=
−
R
T
l
n
K
−
R
T
l
n
K
<
0
R
T
l
n
K
>
0
l
n
K
>
0
⇒
K
>
1
Suggest Corrections
0
Similar questions
Q.
Δ
G
0
is related to K by the relation _____.
Q.
Calculate
Δ
H
0
f
for
U
B
r
4
from
Δ
G
0
of reaction and the
S
0
values.
U
(
s
)
+
2
B
r
2
(
l
)
→
U
B
r
4
(
s
)
;
Δ
G
0
=
−
788.6
K
J
;
S
0
(
J
/
K
−
m
o
l
)
50.3
,
152.3
,
242.6
Q.
With the following information, determine standard Gibb's free energy of formation of
N
2
O
4
(g).
(i)
1
2
N
2
(
g
)
+
1
2
O
2
(
g
)
→
N
O
(
g
)
Δ
G
0
= 86.6 kJ
(ii)
N
O
(
g
)
+
1
2
O
2
(
g
)
→
1
2
N
2
(
g
)
Δ
G
0
= 34.82 kJ
(iii)
2
N
O
2
(
g
)
→
N
2
O
4
(
g
)
Δ
G
0
= 5.77 kJ
Q.
P
C
l
5
(
g
)
→
P
C
l
3
(
g
)
+
C
l
2
(
g
)
at 298 K,
K
c
=
1.8
×
10
−
7
.
What is
Δ
G
0
for the reaction?
Q.
Calculate:
a)
Δ
G
0
.
b) the equilibrium constant for the formation of
N
O
2
from NO and
O
2
at 298 K.
N
O
(
g
)
+
1
2
O
2
(
g
)
⇌
N
O
2
(
g
)
where
Δ
f
G
0
(
N
O
2
)
=
52.0
kJ/mol
Δ
f
G
0
(
N
O
)
=
87.0
kJ/mol
Δ
f
G
0
(
O
2
)
=
0
kJ/mol.
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