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Byju's Answer
Standard XII
Chemistry
Heat of Reaction
2Bs + 3 / 2 O...
Question
2
B
(
s
)
+
3
2
O
_
2
(
g
)
→
B
2
O
3
(
s
.
)
Δ
H
=
−
1273
k
j
H
_
2
(
g
)
+
1
2
O
_
2
(
g
)
→
H
_
2
O
(
l
)
Δ
H
=
−
286
k
j
H
2
O
(
l
)
→
H
2
O
(
g
)
Δ
H
=
44
k
j
2
B
(
s
)
+
3
H
2
(
g
)
→
B
2
H
6
(
g
)
Δ
H
=
365
k
j
B
2
H
6
(
g
)
+
3
O
2
(
g
)
B
2
O
3
(
s
)
+
3
H
2
O
(
g
)
Δ
H
=
?
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Solution
2
B
(
s
)
+
3
2
O
2
(
g
)
→
B
2
O
3
(
s
)
Δ
H
=
−
1273
k
J
Δ
H
B
2
O
3
f
=
−
1273
k
J
(
Δ
H
B
f
=
0
,
Δ
H
O
2
f
=
0
)
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
l
)
Δ
H
=
−
286
k
J
Δ
H
r
e
a
c
t
i
o
n
=
−
286
+
44
=
−
242
k
J
Δ
H
H
2
O
(
g
)
f
=
Δ
H
r
e
a
c
t
i
o
n
=
−
242
k
J
(
Δ
H
H
2
f
=
0
,
Δ
H
O
2
f
=
0
)
H
2
O
(
l
)
→
H
2
O
(
g
)
Δ
H
=
44
k
J
2
B
(
s
)
+
3
H
2
(
g
)
→
B
2
H
6
(
g
)
Δ
H
=
365
k
J
Δ
H
B
2
H
6
f
=
365
k
J
(
Δ
H
B
(
s
)
f
=
0
,
Δ
H
H
2
f
=
0
)
We have to calculate
Δ
H
r
e
a
c
t
i
o
n
for
B
2
H
6
(
g
)
+
3
O
2
(
g
)
B
2
O
3
(
s
)
+
3
H
2
O
(
g
)
Δ
H
r
x
n
=
Δ
H
B
2
O
3
f
+
3
Δ
H
H
2
O
(
g
)
f
−
Δ
H
B
2
H
6
f
⟹
Δ
H
r
x
n
=
−
1273
−
3
×
242
−
365
⟹
Δ
H
r
x
n
=
−
2364
k
J
Suggest Corrections
1
Similar questions
Q.
Diborane is a potential rocket fuel which undergoes combustion according to the reaction
B
2
H
6
(
g
)
+
3
O
2
(
g
)
→
B
2
O
3
(
s
)
+
3
H
2
O
(
g
)
Form the following dada, calculation the enthalpy change for the combustion of diborane.
2
B
(
s
)
+
(
3
/
2
)
O
2
(
g
)
→
B
2
O
3
(
s
)
Δ
H
=
−
1273
k
J
m
o
l
−
1
H
2
(
g
)
+
(
1
/
2
)
O
2
(
g
)
→
H
2
O
(
1
)
Δ
H
=
−
286
k
J
m
o
l
−
1
H
2
O
(
1
)
→
H
2
O
(
g
)
Δ
H
=
44
k
J
m
o
l
−
1
2
B
(
s
)
+
3
H
2
(
g
)
→
B
2
H
6
(
g
)
Δ
H
=
36
K
J
m
o
l
−
1
Q.
2
C
(
s
)
+
2
O
2
(
g
)
→
2
C
O
2
(
g
)
,
Δ
H
=
−
787
k
J
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
l
)
,
Δ
H
=
−
286
k
J
C
2
H
2
(
g
)
+
5
2
O
2
(
g
)
→
2
C
O
2
(
g
)
+
H
2
O
(
l
)
,
Δ
H
=
−
1310
k
J
From the above data, heat of formation of acetylene is:
Q.
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
g
)
;
Δ
H
=
x
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
l
)
;
Δ
H
=
y
Heat of vaporisation of water is:
Q.
Given that:
2
C
(
s
)
+
2
O
2
(
g
)
⟶
2
C
O
2
(
g
)
;
Δ
H
=
−
787
k
J
.
.
.
(
i
)
H
2
(
g
)
+
1
2
O
2
(
g
)
⟶
H
2
O
(
l
)
;
Δ
H
=
−
286
k
J
.
.
.
(
i
i
)
C
2
H
2
(
g
)
+
5
2
O
2
(
g
)
⟶
2
C
O
2
(
g
)
+
3
H
2
O
(
l
)
.
.
.
.
(
i
i
i
)
Δ
H
=
−
1301
k
J
Heat formation of acetylene is:
Q.
The enthalpy of vapourisation of liquid water using the data
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
l
)
;
Δ
H
=
−
285.77
K
J
m
o
l
−
1
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
g
)
;
Δ
H
=
−
241.84
K
J
m
o
l
−
1
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