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Byju's Answer
Standard XII
Chemistry
Heat of Formation
The freezing ...
Question
The freezing point of a solution containing 28.335
c
m
3
of ethylene glycol in 50 g water is found to be
–
34
∘
C. Assuming ideal behaviour, calculate the density of ethylene glycol.
K
f
for water 1.86 K kg
m
o
l
−
1
.
___
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Solution
W
e
t
h
y
l
e
n
e
g
l
y
c
o
l
=
M
2
×
Δ
T
f
×
W
w
a
t
e
r
1000
×
k
f
=
62
×
34
×
50
1000
×
1.86
=
56.67
g
d
=
W
V
=
56.67
28.335
=
2
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Similar questions
Q.
The freezing point of a solution containing 28.335
c
m
3
of ethylene glycol in 50 g water is found to be
–
34
∘
C. Assuming ideal behaviour, calculate the density of ethylene glycol.
K
f
for water 1.86 K kg
m
o
l
−
1
.
___
Q.
The freezing point of a solution containing
50
cm
3
of ethylene glycol in
50
g
of water is found to be -34°C. Assuming ideal behaviour, calculate the density of ethylene glycol in
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(
K
f
for water
=
1.86
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−
1
)
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The freezing point of a solution containing
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. Assuming ideal behaviour, the density of ethylene glycol
(
K
f
for water
=
1.86
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k
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Q.
The freezing point of a solution
50
c
m
3
of ethylene glycol in
50
g
water is found to be
−
34
∘
C
. Assuming ideal behaviour, calculate the density of ethylene glycol
(
K
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H
2
O
=
1.86
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1
)
Given:
Molar mass of Ethylene glycol
=
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g
m
o
l
−
1
Q.
The freezing point of a solution containing
50
cm
3
of ethylene glycol in
50
g
of water is found to be
−
34
∘
C
. Assuming ideal behaviour, calculate the density of ethylene glycol. (
K
f
for water
=
1.86
K kg mol
−
1
)
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