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Byju's Answer
Standard XII
Chemistry
Enthalpy of Combustion
For the react...
Question
For the reaction at
300
K
A
(
g
)
+
B
(
g
)
→
C
(
g
)
;
Δ
E
=
−
3.0
kcal;
Δ
S
=
−
10.0
cal/K value of
Δ
G
is:
A
−
600
cal
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B
−
6600
cal
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C
−
6000
cal
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D
None
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Solution
The correct option is
D
None
For the reaction
A
(
g
)
+
B
(
g
)
→
C
(
g
)
T
=
300
K
;
Δ
E
=
Δ
U
−
3.0
kcal;
Δ
S
=
−
10.0
cal/K
Δ
G
=
Δ
H
−
T
Δ
S
Δ
H
=
Δ
U
+
Δ
n
g
R
T
Δ
H
=
−
3000
+
(
1
−
2
)
×
1.987
×
300
Δ
H
=
−
3594
c
a
l
thus
Δ
G
=
−
3594
−
300
×
(
−
10
)
Δ
G
=
−
594
c
a
l
Suggest Corrections
0
Similar questions
Q.
For this reaction at 300 K
A
(
g
)
+
B
(
g
)
→
C
(
g
)
△
U
=
−
3.0
k
c
a
l
;
△
S
=
−
10.0
c
a
l
/
K
value of
△
G
is :
Q.
For this reaction at 300 K
A
(
g
)
+
B
(
g
)
→
C
(
g
)
△
U
=
−
3.0
k
c
a
l
;
△
S
=
−
10.0
c
a
l
/
K
value of
△
G
is :
Q.
If
Δ
G
and
Δ
S
for the reaction:
A
(
g
)
+
B
(
g
)
→
P
(
g
)
, at 300 K are
−
600
cal and
−
10
c
a
l
/
K
. Then
Δ
H
for the reaction in kcal is ______.
Q.
For the reaction at
300
K,
A
(
g
)
+
B
(
g
)
→
C
(
g
)
△
E
=
−
3.0
k
c
a
l
;
△
S
=
−
10.0
cal/K, then the value of
△
G
is:
Q.
For the reaction at
300
K
A
(
g
)
+
B
(
g
)
→
C
(
g
)
Δ
H
=
−
3.0
k
c
a
l
;
Δ
S
=
−
10.0
c
a
l
/
K
value of
Δ
G
is:
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