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Byju's Answer
Standard XII
Chemistry
Gibbs Free Energy & Spontaneity
For the given...
Question
For the given reaction,
H
2
(
g
)
+
C
l
2
(
g
)
⟶
2
H
+
(
a
q
)
+
2
C
l
−
(
a
q
)
;
Δ
G
0
=
−
262.4
k
J
The value of free energy of formation
(
Δ
G
0
f
)
for the ion
C
l
−
1
(
a
q
)
, therefore will be:
A
−
131.2
k
J
m
o
l
−
1
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B
+
131.2
k
J
m
o
l
−
1
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C
−
262.4
k
J
m
o
l
−
1
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D
+
262.4
k
J
m
o
l
−
1
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Solution
The correct option is
A
−
131.2
k
J
m
o
l
−
1
(
Δ
G
0
)
reaction
=
Δ
G
0
f
(Products)
−
Δ
G
0
f
(reactants)
∴
264.4
=
[
2
Δ
G
0
f
(
H
+
)
+
2
Δ
G
0
f
(
C
1
−
)
]
or
264.4
=
−
[
Δ
G
0
f
(
H
2
)
+
Δ
G
0
f
(
C
l
2
)
]
=
[
0
+
2
Δ
G
0
f
(
C
l
−
)
]
+
[
0
+
0
]
or,
−
262.4
=
2
Δ
G
0
f
(
C
l
−
)
or,
Δ
G
0
f
(
C
l
−
)
=
−
131.2
k
J
m
o
l
−
1
Suggest Corrections
0
Similar questions
Q.
The standard free energy of formation for
A
g
C
l
at
298
K
is
−
109.7
k
J
m
o
l
−
1
.
Δ
G
o
(
A
g
+
)
=
77.2
k
J
/
m
o
l
;
Δ
G
o
(
C
l
−
)
=
−
131.2
k
J
/
m
o
l
. Find the solubility of
A
g
C
l
in
0.05
M
K
C
l
. Neglect any complication due to complexation.
Q.
Calculate the lattice enthalpy of
C
a
C
l
2
, given that :
Enthalpy of sublimation for
C
a
(
s
)
→
C
a
(
g
)
=
121
k
J
m
o
l
−
1
Enthalpy of dissociation of
C
l
2
(
g
)
→
2
C
l
(
g
)
=
242.8
k
J
m
o
l
−
1
Ionisation energy of
C
a
(
g
)
→
C
a
+
+
(
g
)
=
2422
k
J
m
o
l
−
1
Electron gain enthalpy of
2
C
l
→
2
C
l
−
1
=
(
2
×
−
355
)
k
J
m
o
l
−
1
=
−
710
k
J
m
o
l
−
1
Enthalpy of formation of
C
a
C
l
2
=
−
795
k
J
m
o
l
−
1
Q.
Consider the following reactions.
(a)
H
+
(
a
q
)
+
O
H
−
(
a
q
)
=
H
2
O
(
l
)
,
Δ
H
=
−
X
1
kJ
m
o
l
−
1
(b)
H
2
(
g
)
+
1
2
O
2
(
g
)
=
H
2
O
(
l
)
,
Δ
H
=
X
2
kJ
m
o
l
−
1
(c)
C
O
2
(
g
)
+
H
2
(
g
)
=
C
O
(
g
)
+
H
2
O
(
l
)
−
X
3
kJ
m
o
l
−
1
(d)
C
2
H
2
(
g
)
+
5
2
O
2
(
g
)
=
2
C
O
2
(
g
)
+
H
2
O
(
l
)
+
X
4
kJ
m
o
l
−
1
Enthalpy of formation of
H
2
O
(
l
)
is:
Q.
What will be
Δ
H
for the reaction,
C
H
2
C
l
2
→
C
+
2
H
+
2
C
l
?
(B.E. of C - H and C - Cl bonds are 416 kJ
m
o
l
−
1
and 325 kJ
m
o
l
−
1
respectively)
Q.
For the reaction
N
2
+
3
X
2
→
2
N
X
3
where
X
=
F
,
C
l
(the average bond energies are
F
−
F
=
155
k
J
m
o
l
−
1
,
N
−
F
=
272
k
J
m
o
l
−
1
,
C
l
−
C
l
=
242
k
J
m
o
l
−
1
,
N
−
C
l
=
200
k
J
m
o
l
−
1
and
N
≡
N
=
941
k
J
m
o
l
−
1
). The heats of formation of
N
F
3
and
N
C
l
3
in
k
J
m
o
l
−
1
, respectively, are closest to:
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