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Question
Chemistry
For the given reactions, H 2(g)+ F 2(g) arrow 2 HF (g) ; , Δ H°=-124 kcal H 2(g) arrow 2 H (g) ; Δ H°=104 kcal F2(g) arrow 2 F(g);, Δ H°=37.8 kcal then the value of Δ H° for H (g)+ F (g) arrow HF (g) is
Q. For the given reactions,
H
2
(
g
)
+
F
2
(
g
)
→
2
H
F
(
g
)
;,
Δ
H
∘
=
−
124
k
c
a
l
H
2
(
g
)
→
2
H
(
g
)
;
Δ
H
∘
=
104
k
c
a
l
F
2
(
g
)
→
2
F
(
g
)
;,
Δ
H
∘
=
37.8
k
c
a
l
then the value of
Δ
H
∘
for
H
(
g
)
+
F
(
g
)
→
H
F
(
g
)
is
2275
156
Thermodynamics
Report Error
A
142
k
c
a
l
B
−
132.9
k
c
a
l
C
132
k
c
a
l
D
134
k
c
a
l
Solution:
For the reaction,
H
2
(
g
)
+
F
2
(
g
)
→
2
H
F
(
g
)
;,
Δ
H
∘
=
−
124
k
c
a
l
Δ
H
∘
=
Σ
B
.
E
.
(reactants)
−
Σ
B
.
E
.
(products)
or
−
124
=
Δ
H
H
−
H
+
Δ
H
F
−
F
−
2Δ
H
H
−
F
=
104
+
37.8
−
2Δ
H
H
−
F
∴
2Δ
H
H
−
F
∘
=
104
+
37.8
+
124
=
265.8
k
c
a
l
Bond energy of
H
−
F
=
2
265.8
=
132.9
k
c
a
l
∴
Δ
H
∘
for the given reaction
=
−
132.9
k
c
a
l