Post on 23-Jan-2020
a. Water (A)–Glycerol (B) System
P ¼ 101.3 kPa
Data of Chen and Thompson, J. Chem. Eng. Data, 15, 471 (1970)
Temperature, (C yA xA aA,B
100.0 1.0000 1.0000
104.6 0.9996 0.8846 333
109.8 0.9991 0.7731 332
128.8 0.9980 0.4742 544
148.2 0.9964 0.3077 627
175.2 0.9898 0.1756 456
207.0 0.9804 0.0945 481
244.5 0.9341 0.0491 275
282.5 0.8308 0.0250 191
290.0 0.0000 0.0000
b. Methanol (A)–Water (B) System
P ¼ 101.3 kPa
Data of J.G. Dunlop, M.S. thesis, Brooklyn Polytechnic
Institute (1948)
Temperature, (C yA xA aA,B
64.5 1.000 1.000
66.0 0.958 0.900 2.53
69.3 0.870 0.700 2.87
73.1 0.779 0.500 3.52
78.0 0.665 0.300 4.63
84.4 0.517 0.150 6.07
89.3 0.365 0.080 6.61
93.5 0.230 0.040 7.17
100.0 0.000 0.000
c. Para-xylene (A)–Meta-xylene (B) System
P ¼ 101.3 kPa
Data of Kato, Sato, and Hirata, J. Chem. Eng. Jpn., 4, 305 (1970)
Temperature, (C yA xA aA,B
138.335 1.0000 1.0000
138.491 0.8033 0.8000 1.0041
138.644 0.6049 0.6000 1.0082
138.795 0.4049 0.4000 1.0123
138.943 0.2032 0.2000 1.0160
139.088 0.0000 0.0000
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a. Methanol (A)–Water (B) System
T ¼ 50(C
Data of McGlashan and Williamson, J. Chem. Eng. Data, 21,
196 (1976)
Pressure, psia yA xA aA,B
1.789 0.0000 0.0000
2.373 0.2661 0.0453 7.64
3.369 0.5227 0.1387 6.80
4.641 0.7087 0.3137 5.32
5.771 0.8212 0.5411 3.90
6.811 0.9090 0.7598 3.16
7.800 0.9817 0.9514 2.74
8.072 1.0000 0.0000
b. Methanol (A)–Water (B) System
T ¼ 150(C
Data of Griswold and Wong, Chem. Eng. Prog. Symp. Ser.,
48(3), 18 (1952)
Pressure, psia yA xA aA,B
73.3 0.060 0.009 7.03
85.7 0.213 0.044 5.88
93.9 0.286 0.079 4.67
139.7 0.610 0.374 2.62
160.4 0.731 0.578 1.98
193.5 0.929 0.893 1.57
196.5 0.960 0.936 1.64
199.2 0.982 0.969 1.75
c. Methanol (A)–Water (B) System
T ¼ 250(C
Data of Griswold and Wong, Chem. Eng. Prog. Symp. Ser.,
48(3), 18 (1952)
Pressure, psia yA xA aA,B
681 0.163 0.066 2.76
818 0.344 0.180 2.39
949 0.487 0.331 1.92
1099 0.643 0.553 1.46
1204 0.756 0.732 1.13
1219 0.772 0.772 1.00
1234 0.797 0.797 1.00
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100
90
80
70
60
50
200
150
100
50
1.0
0.8
0.6
0.4
0.2
0.00 0.2 0.4
Saturated liquid
Saturated vapor
Mole fraction of methanol in liquid, x, or vapor, y
(a)
0.6 0.8 1
Te
mp
era
ture
, C
0 0.2 0.4
Mole fraction of methanol in liquid
(b)
0.6 0.8 1Mo
le f
racti
on
of
me
tha
no
l in
va
po
r
0 0.2 0.4
Mole fraction of methanol in liquid
0.6 0.8 1
Sy
ste
m p
ressu
re,
psia
(c)
Vapor–liquid equilibrium conditions for the methanol–water system: (a) T–y–x diagram for 1 atm pressure; (b) y–x diagram for 1 atmpressure; (c) P–x diagram for 150(C.
275
250
225
200
175
150
135
121.1
107.2
93.3
79.4
65.60 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9
Vapor
Liquid
G
E
A
D
B
F
C
H
Saturated vapor
Saturated liquid
1.0
Mole fraction n-hexane, x or y
Te
mp
era
ture
, °F
Te
mp
era
ture
, °C
yA ¼aA;BxA
1þ xAðaA;B " 1Þ
1
0.8
0.6
0.4
0.2
00 0.2 0.4
1,2 =
5
α
0.6
1
1.25
1.5
2
3
0.8 1
Mole fraction of component 1 in liquid, x
Mo
le f
racti
on
of
co
mp
on
en
t in
va
po
r, y
Fondamenti delle operazioni unitarie dell'industria chimica - Diagrammi e tabelle 2015
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1.00.80.6
Mole fraction isopropyl etherin liquid phase, x1
(b)
Mole fraction isopropyl ether
in liquid phase, x1
(a)
Equilibrium line
Reference line, y1 = x1
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
0.40.2
050
60
70
80
90
100
0.2 0.4
Te
mp
era
ture
, °C
0.6
Vapor
Liquid
Vapor + liquid
Bubble-point line
Dew-point line
Mole fraction isopropyl ether
(c)
0.8 1.0
00 0.2 0.4 0.6 0.8 1.0
Mo
le f
racti
on
iso
pro
py
l e
the
rin
va
po
r p
ha
se
, y
1
0
100
200
300
400
500
600
700
800
900
1000
13
26
40
53
66
80
93
106
119
133
Pre
ssu
re,
torr
Pre
ssu
re,
kP
a
Tota
l pre
ssure
Partialpressure of
alcohol P2
isopropyl
of isopropyl ether P1
Partial p
ressure
Minimum-boiling-point azeotrope,isopropyl ether–isopropyl alcoholsystem: (a) partial and total pressures at70(C; (b) vapor–liquid equilibria at 101 kPa; (c) phase diagram at 101 kPa.[Adapted from O.A. Hougen, K.M.
Watson, and R.A. Ragatz, Chemical
Process Principles. Part II, 2nd ed., JohnWiley & Sons, New York (1959).]
1.0
Total pressure
of ace
tone p
1
0 0.2 0.4
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
0.6
Mole fraction acetonein liquid phase, x1
Equilibrium line
Reference line,y1 = x1
0.8 1.0
0 0.20
10
20
30
40
50
60
70
80
90
100
0.4 0.6
Mole fraction acetone
Mo
le f
racti
on
ace
ton
ein
va
po
r p
ha
se
, y
1
Te
mp
era
ture
, °C
Liquid
Vapor + liquid
Vapor
Dew-point line
Bubble-point line
(c)
0.8 1.0
0.80.6
Mole fraction acetonein liquid phase, x1
Pre
ssu
re,
torr
Pre
ssu
re,
kP
a
(b)(a)
0.40
100
200
300
400
500
600
700
800
900
1000
13
26
40
53
66
80
93
106
119
133
0.20
P
artia
l pre
ssrue
Partial pressure
of chloroof rm
p2
Maximum-boiling-point azeotrope,acetone–chloroform system:
(a) partial and total pressures at 60(C;
(b) vapor–liquid equilibria at 101 kPa;
(c) phase diagram at 101 kPa pressure.
[Adapted from O.A. Hougen, K.M.
Watson, and R.A. Ragatz, Chemical
Process Principles. Part II, 2nd ed., John
Wiley & Sons, New York (1959).]
1.0
0.8
0.6
0.4
0.2
0
y eth
yl a
lco
ho
l
0 0.2 0.4 0.6
Equilibrium
45° line
1 atm
0.8 1.0
xethyl alcohol
Equilibrium curve for n-hexane/ethanol.
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C08 09/20/2010 Page 319
xC = 0.8
xC = 0.7
xC = 0.6
xC = 0.5
xC = 0.4
xC = 0.3
xC = 0.2
xC = 0
A′
M
F
Tie
lin
e
Phase envelope
Raffinate
Extract 1
0
Wt f
ract
ion C
xC = 0.9
xC = 0.1
1.0
0.9
0.8
0.7
0.6
0.5
0.4
0.3
0.2
0.1
00 0.1
S
CA
0.2 0.3 0.4 0.50 1
Wt
frac
tio
n S
01
0.6 0.7 0.8 0.9 1.0
A′′
Plaitpoint
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Water(A)
Ethylene Glycol(B)
Furfural(C)
0.10.9
0.20.8
0.30.7
0.40.6
0.5
Mass fra
ction w
ate
r
0.5
Mass
fra
ctio
n e
thyle
ne g
lyco
l
0.60.4
0.70.3
0.80.2
0.90.1
0.9 0.8 0.7 0.6 0.5 0.4 0.3 0.2 0.1
Mass fraction furfural
(a)
Plait
R
M
E
D G
Ext
ract
P
Point M
iscibility boundary
Raffin
ate
Tie line
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1.0
Mass fraction furfural
(b)
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
Ma
ss f
racti
on
gly
co
l
Extract
Raff
inate
RP
M
E0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1.0
Mass fraction glycol in raffinate
(c)
0.1
0
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
Ma
ss f
racti
on
gly
co
l in
ex
tra
ct
P
E
R
45° L
ine
Liquid–liquid equilibrium, ethylene glycol–furfural–water, 25(C, 101 kPa: (a) equilateral-triangular diagram; (b) right-triangular diagram; (c) equilibrium solute diagram in mass fractions; (continues )
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0 1 2 3 4 5
Glycol/water in raffinate
(d)
0.1
0
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
Gly
co
l/fu
rfu
ral
in e
xtr
act
P
E
R
Fu
rfu
ral/
(gly
co
l +
wa
ter)
20
18
16
14
12
10
8
6
4
2
00 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9
Tie li
nes
R
M
E
P
Glycol/(glycol + water)
(e)
(d) equilibrium solute diagram in mass ratios; (e) Janeckediagram.
Equilibrium Miscibility Data in Weight Percent forthe Furfural–Ethylene Glycol–Water System at 25(C and 101 kPa
Furfural Ethylene Glycol Water
95.0 0.0 5.0
90.3 5.2 4.5
86.1 10.0 3.9
75.1 20.0 4.9
66.7 27.5 5.8
49.0 41.5 9.5
34.3 50.5 15.2
27.5 52.5 20.0
13.9 47.5 38.6
11.0 40.0 49.0
9.7 30.0 60.3
8.4 15.0 76.6
7.7 0.0 92.3
Mutual Equilibrium (Tie-Line) Data for the Furfural–EthyleneGlycol–Water System at 25(C and 101 kPa
Glycol in Water Layer, wt% Glycol in Furfural Layer, wt%
41.5 41.5
50.5 32.5
52.5 27.5
51.5 20.0
47.5 15.0
40.0 10.0
30.0 7.5
20.0 6.2
15.0 5.2
7.3 2.5
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0
6
4
2
68
4
2
68
4
2
68
4
2
68
4
2
10 20 30 40 50Temperature, °C
60 70 80 90 100
O2
H
10–1
10–2
10–3
10–4
10–5
1V
alu
es o
f
, m
ole
fra
ctio
n p
er a
tmo
sph
ere
CH4
H2
N2
C2H6
C2H4
CO2
SO2
NH3
H2S
H2S
Cl2
Cl2
Br2
CO
Henry’s law constant for solubility of gases in water.
[Adapted from O.A. Hougen, K.M. Watson, and R.A. Ragatz, Chemical Pro-
cess Principles. Part I, 2nd ed., John Wiley & Sons, New York (1954).]
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(a)
x B, M
ass
solu
te/m
ass
of
liqu
id
xA, Mass of solid/mass of liquid
U
Un
der
flo
w
Ove
rflo
w
F
M
S 1.0
V
Tie line
1.0
0.8
0.6
0.4
0.2
0
x B, M
ass
solu
te/m
ass
of
liqu
id
xA, Mass of solid/mass of liquid
U
Ove
rflo
w
F
M
S 1.0
V
Tie line
1.0
0.8
0.6
0.4
0.2
0
Underflow
(b)
Figure 4.20 Underflow–overflow conditions for ideal leaching:
(a) constant-solution underflow; (b) variable-solution underflow.
MIXER-SETTLER
Solid feed, F
Insoluble ASolute B
Overflow, V
LiquidB, C
Underflow, U
LiquidB, C
SolidA
Liquidsolvent, S
C
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Pressure, psia
K-v
alu
e
100 1000 10,000
100
10
1.0
.01
.1
Experimental dataof Yarborough
S–R–K correlation
Temperature 250°F
N2
C1
CO2
C2
C3
nC5
nC7
Toluene
nC10
H2S
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Equi
libri
um
Gas inF = (A + P)= 2 mmol
zF = P/ (A + P) = 0.5
Gas outG = (A + P)= 1 mmol
y* = P/ (P + A)
Stage
S, g solidx* = P/(P + A)
W = P + A =1 mmol
x* = 0.365y* = 0.635
y*
x*
yyyy
x
x
y = 1 – x
S, g solid
0.9
0.8
0.7
0.6
0.5
0.4
0.3
0.2
0.1
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1.0
Mo
le f
ract
ion
pro
pan
e in
gas
, y
Mole fraction propane in adsorbate, x
(a)
2.4
2.3
2.0
1.9
1.8
1.7
1.6
1.50 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1.0
mm
ole
ad
sorb
ate/
g a
dso
rben
t
Mole fraction propane in adsorbate, y, x
(b)
Figure 4.29 Adsorption equilibrium at 25�C and 101 kPa of
propane and propylene on silica gel.
[Adapted from W.K. Lewis, E.R. Gilliland, B. Chertow, and W. H. Hoffman,
J. Am. Chem. Soc, 72, 1153 (1950).]
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2000
50
100
150
200
250
300
350
400
220 240 260 280 300 320 340Temperature, K
Solid Liquid
Triple point
Pres
sure
, bar
Gas
Critical point
Supercritical-
fluidregion
0 5 10
Pressure, MPa
Co
nce
ntr
atio
n o
f so
lute
in
gas
ph
ase,
g/L
100
50298 K
10
5
1
0.5
0.1
0.05
0.01
Effect of pressure on solubility of pICBin supercritical ethylene.
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C2H5OH
H2O C 2O
Figure 11.43 Liquid–fluid equilibria for CO2–C2H5OH–H2O at
308–313.2 K and 10.1–10.34 MPa.
Critical
Temperature,
Critical
Pressure,
Critical
Density,
Solvent K MPa kg/m3
192 4.60 162
283 5.03 218
304 7.38 468
305 4.88 203
365 4.62 233
370 4.24 217
406 11.3 235
Methane
Ethylene
Carbon dioxide
Ethane
Propylene
Propane
Ammonia
Water 647 22.0 322
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