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Byju's Answer
Standard XII
Physics
Calorimetry
Which of the ...
Question
Which of the following relationships is not correct for the reaction between
Δ
H
and
Δ
U
?
A
When
Δ
n
g
= 0 then
Δ
H
=
Δ
U
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B
When
Δ
n
g
> 0 then
Δ
H
>
Δ
U
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C
When
Δ
n
g
< 0 then
Δ
H
<
Δ
U
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D
When
Δ
n
g
R
T
= 0 then
Δ
H
>
Δ
U
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Solution
The correct option is
B
When
Δ
n
g
R
T
= 0 then
Δ
H
>
Δ
U
The relation between
Δ
H
and
Δ
U
is given as:
Δ
H
=
Δ
U
+
Δ
(
P
V
)
i.e.,
Δ
H
=
Δ
U
+
Δ
n
g
R
T
∴
For
Δ
n
g
=
0
,
Δ
H
=
Δ
U
∴
For
Δ
n
g
>
0
,
Δ
H
=
Δ
U
+
Δ
n
g
R
T
∴
For
Δ
n
g
<
0
,
Δ
H
=
Δ
U
−
Δ
n
g
R
T
∴
For
Δ
n
g
R
T
=
0
,
Δ
H
=
Δ
U
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0
Similar questions
Q.
In the relation
Δ
H
=
Δ
U
+
(
Δ
n
g
)
R
T
the units of
Δ
n
g
is mol.If true enter 1 else o
Q.
The difference of
Δ
H
−
Δ
U
for the given reaction is
Δ
n
g
R
T
. The value of
Δ
n
g
is _____ .
C
6
H
12
O
6
(
s
)
+
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O
2
(
g
)
⟶
+
6
C
O
2
(
g
)
+
6
H
2
O
(
v
)
Q.
For gaseous reactions, if
Δ
H
is the change in enthalpy and
Δ
U
that in internal energy, then
Δ
H
is always greater than
Δ
U
.
If true 1 else 0.
Q.
For which reaction,
Δ
H
>
Δ
U
? (
Δ
H
=
change in enthalpy,
Δ
U
=
change in internal energy )
Q.
Two mole of ideal diatomic gas
(
C
v
,
m
=
5
2
R
)
at 300 K and 5 atm expanded irreversly and adiabatically to a final pressure of 2 atm against a constant pressure of 1 atm. Calculate q, w,
Δ
H
and
Δ
U
.
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