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Byju's Answer
Standard XI
Chemistry
Depression in Freezing Point
The mass of b...
Question
The mass of benzene which can freeze out on addition of 7.3 g of triphenyl methane to 1000 g of benzene at a temperature of
0.2
∘
C
less than the normal freezing point of benzene is
(
K
f
(
C
6
H
6
)
=
5.12
K
k
g
m
o
l
–
1
)
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Solution
Δ
T
f
=
K
f
m
⇒
0.2
=
5.12
7.3
×
1000
244
×
w
(
M
t
r
i
p
h
e
n
y
l
m
e
t
h
a
n
e
=
244
)
w = mass of benzene = 766
Mass of benzene freezed out= 1000-766
= 234 g
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Q.
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On dissolving 0.5 g of a non-volatile non-ionic solute in 39 g of benzene, its vapour pressure decreases from 650 mm of Hg to 640 mm of Hg. The depression in freezing point of benzene (in K) upon addition of the solute is: ( Given: The molar mass and the molal freezing point depression constant for benzene are
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Q.
Addition of
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k
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Addition of
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