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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)


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)


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

Fondamenti delle operazioni unitarie dell'industria chimica - Diagrammi e tabelle 2015

1

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)


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)


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


2

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


3

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.


4


5

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


6

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 )


7

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


8


9

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).]


10

(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


11

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


12

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).]


13


14


15


16


17


18


19


20


21

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.


22

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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