Vapour pressure of chloroform (CHCI) and dichloromethane (CH,CI)
at 999 Rare 200 mm Hg and 415 mm Hg respectively. 6) Calculate
the vapour pressure of the solution prepared by mixing 25.5 g of
CHCI, and 40 g of CH CI, at 298 K and, (10) mole fractions of each
component in vapour phase
Answers
Answered by
2
ANSWER
Vapour pressure of pure chloroform = P
A
o
=200mm
Vapour pressure of pure dichloromethane P
B
o
=415mmHg
Molar mass M
A
=119.5g
Molar mass M
B
=85g
(i) mass of CHCl
3
=25.5g
number of mole =
119.5
25.5
=0.213
Mass of CH
2
Cl
2
=40g
Number of mole =
85
40
=0.47
x
A
=
0.213+0.47
0.213
=0.322
x
B
=1−0.322=0.688
P=P
A
o
X
A
+P
B
o
x
B
=200×0.322+415×0.688
=64.4+285.52=349.92
(ii) Mole fraction of chlotoform = 0.322
Mole fraction of CH
2
Cl
2
=0.688
Similar questions