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Byju's Answer
Standard XII
Chemistry
Heat of Reaction
For the react...
Question
For the reaction,
C
2
H
4
(
g
)
+
3
O
2
→
2
C
O
2
(
g
)
+
2
H
2
O
(
l
)
;
Δ
U
=
−
1415
kJ. Then
Δ
H
at
27
o
C is?
A
−
1410
kJ
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B
−
1420
kJ
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C
+
1420
kJ
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D
+
1410
kJ
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Solution
The correct option is
B
−
1420
kJ
For a chemical reaction-
Δ
H
=
Δ
E
+
Δ
n
g
R
T
Δ
H
=
−
1415
+
−
2
×
8.314
×
300
=
−
1420
K
J
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0
Similar questions
Q.
Given that:
C
(
s
)
+
O
2
(
g
)
→
C
O
2
(
g
)
;
Δ
H
=
−
394
kJ and
2
H
2
(
g
)
+
O
2
(
g
)
→
2
H
2
O
(
l
)
,
Δ
H
=
−
568
kJ and
C
2
H
5
O
H
(
l
)
+
3
O
2
(
g
)
→
2
C
O
2
(
g
)
+
3
H
2
O
(
l
)
;
Δ
H
=
−
1058
kJ/mole. Using the data, the heat of formation of ethanol is:
Q.
The heat of formation of
C
O
2
(
g
)
is -394 kJ/mole and that of
H
2
O
(
l
)
is -286 kJ/mole. The heat of combustion of
C
2
H
4
is -1412 kJ/mole. What is the heat of formation of
C
2
H
4
?
C
2
H
4
(
g
)
+
3
O
2
(
g
)
→
2
C
O
2
(
g
)
+
2
H
2
O
(
l
)
Q.
I
.
E
a
=
15
k
J
m
o
l
−
1
;
Δ
H
=
−
70
k
J
m
o
l
−
1
I
I
.
E
a
=
30
k
J
m
o
l
−
1
;
Δ
H
=
−
15
k
J
m
o
l
−
1
I
I
I
.
E
a
=
60
k
J
m
o
l
−
1
;
Δ
H
=
+
20
k
J
m
o
l
−
1
If above reactions are at same frequency factor and temperature, then fastest and slowest reactions are:
Q.
Using the data provided, calculate the multiple bond energy
(
k
J
m
o
l
−
1
)
of a
C
≡
C
bond in
C
2
H
2
.
Given that the heat of formation of
C
2
H
2
=
225
k
J
m
o
l
−
1
.
(take the bond energy of
C
−
H
bond as
350
k
J
m
o
l
−
1
):
2
C
(
s
)
→
2
C
(
g
)
△
H
=
1410
k
J
m
o
l
−
1
H
2
(
g
)
→
2
H
(
g
)
△
H
=
330
k
J
m
o
l
−
1
Q.
H
2
(
g
)
+
1
2
O
2
(
g
)
⟶
2
H
2
O
(
l
)
;
Δ
H
=
−
86
k
J
2
H
2
(
g
)
+
O
2
(
g
)
⟶
2
H
2
O
(
l
)
.
.
.
.
.
.
.
.
.
k
J
(
±
?
)
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