Upload
bahman-homayun
View
214
Download
0
Embed Size (px)
Citation preview
7/26/2019 Industrial & Engineering Chemistry Volume 45 Issue 1 1953 Pigford, R. L. -- Absorption and Humidification
1/5
ABSORPTION A
HUMIDIFICATI
ms
R
L.
PIGFORD
UNIVERSITY
OF
DELAWARE NEWARK,
DEL.
r*
Impor tant progress in gas absorpt ion has been made in the f ields of phase equi l ibr ia, especial ly
for hyd rocarbon systems, and i n s tudies
of
packed towers.
O n ly a few papers have appeared
in the pract ical ly m ore important f ield of t ray-tower performance.
CCURATE and reliable methods of correlating and predicting
phase equilibrium data for gas-liquid systems must be made
& Available before general design procedures
for
gas-liquid con-
tact ing equipment can be developed. Although generalized meth-
ods for estimating gas solubility are not yet available for com-
pounds which differ chemically from the solvent, there has been
substant ial progress in the last few years on methods of esti-
mating phase distribution constants for hydrocarbon systems.
Methods for estimating equilibrium vaporization constants
for light hydrocarbons have been described previously by Bene-
dict, Webb, and Rubin
5 )
ased on an equation of stat e fitted
to
P-TI-T data on pure hydrocarbons. The calculations are rathe r
tedious but the results have been shown to be in bet ter agreement
with existing vapor-liquid equilibrium data tha n many less funda-
mental methods th at have been popular for many years. The
Benedict equation has now been used to calculate th e fugacities of
the hydrocarbons, methane through heptan e, in gas
or
liquid
mixtures and the resulting values of
K
have been correlated
graphically with temperature, pressure,
and composition-ex-
pressed by the molal average normal boiling point of the mix-
ture-by Benedict, Webb, Rubin , and Friend
(6).
Sample
chart s are given in the published article and the complete collec-
tion of c harts for the seven hydrocarbons a t pressures up to
3000
pounds per square inch can be purchased from the
hl.
W. Kellogg
Co.
of
New York City.
As an example of the success of the correlation, the est imated
K values were shown to agree with the data of Webber 37) for
hydrocarbon solubilities in an absorption oil, a t pressures up to
2000
pounds per square inch, the average absolute deviation for
methane being only
7.7%.
The charts published by t he Kellogg
Co. are concluded to bereliable except ( a )when better t han 5%
accuracy is required,
( b )
when the pressure is within 50 pounds
per square inch of the tru e critical pressure of either phase, c )
when the characterization fac tor of either phase is less than
11.4
( d )
when either phase contains more than 30% of a polar com-
pound,
or ( e )
when extensive extrapolation is required beyond
the range of the char ts.
An alternative method of expressing methane solubili ties was
also proposed by Organick and Brown 27) who employed an
empirical relationship based on critical pressures for methane
binary systems, t he correlating pressure
for
any mixture of paraf-
fin hydrocarbons, binary or complex, being defined in terms of
three other variables: the equilibrium pressure, functions of the
equilibrium vapor, and liquid-phase compositions. The liquid
phase is assigned an equivalent molecular weight which is a func-
tion of its boiling point for paraffinic and olefinic compounds and
is also a function of the characterization factor for naphthenics,
aromatics, and other nonparafis of high molecular weight.
Experimental data agreed with values indicated by the correla-
tion in all ranges of t emperature and pressure, within the experi-
mental uncertainty.
Solubilities of methane, ethylene, and isobutane in high-molec-
*
ular-weight paraffinic, naphthenic
and aromatic compounds and in
two complex hydrocarbon absorption oils were de termined
experimentally by Solomon
(36)
and were compared with the
predictions of Benedict, Webb, Rubin, and Friend (6) based on
the Kellogg equation of state. The predictions were made fo
mixtures of paraffin hydrocarbons. It
was found tha t the experi
mental and predicted values agreed if the Watson characteriza-
tion factor ( K ) f the whole liquid phase was greater than about
13
but for smaller K-factors the equilibrium vaporization constants
were larger by a factor as large as 2.4 and 1.9 for methane an d
ethylene, respectively, in
a
liquid having
K
=
10.
The correc
tion charts proposed by Solomon are consistent with the previous
data of Kirkbride and Bertetti (88) and Webber 37) .
A discussion of t he paper by Solomon
(36)
presented by Organ
ick showed that the empirical methods described
in
his pape
with Brown
27)
were nearly
as
effective as the modified Kellogg
procedure described by Solomon.
New data on the methane-isopentane system were published
by Amick, Johnson, and Dodge
2 ) .
Arnold
(3 )
discussed
vaporization equilibria of methane a t high pressures, sunlmariz
ing existing data.
Winn (40) ublished a nomographic repre
sentation of hydrocarbon vapor-liquid equilibria.
Baldwin and Daniel
( 4 )
described experimental measurements
of gas solubility in viscous liquids. Bunsen solubility coefficient
determined by their method for air oxygen and nitrogen in water
were shown to be consistent with reliable data already existing
and new values of gas solubility were reported for permanen
gases in light hydrocarbons.
EQUIPMENT PERFORMANCE
Packed
Towers.
Ergun 14) eviewed data from severa
sources on pressure drop across random packings and compared
them with an equation proposed previously by Ergun and Orning
(16). Only single-phase flow, either liquid or gaseous, through
the solid packing was considered.
As a result it was found th at the equation
represents the
640
experimental points, including data for Ra
schig rings and Berl saddles, with remarkable accuracy, as shown
by Figure 1. The left-hand side of the equation is the friction
factor defined as th e ratio of, the head loss, due to friction, to t h
value of a velocity head based on the tru e fluid velocity,
U / E
between the packing. The first term on the right is caused by
viscous shear an d the second represents the effect of changes i
fluid direction and of flow channel area. In the limit where th
first term predominates, the equation is identical with that o
Kozeny
(28)
nd Carman IO),while at high Reynolds number
the equation reduces to th at of Burke a nd Plummer
(8).
Th
effect
of
free space, e, is in agreement w ith the authors own dat
taken a t various bed expansions using the same solid particles
19
7/26/2019 Industrial & Engineering Chemistry Volume 45 Issue 1 1953 Pigford, R. L. -- Absorption and Humidification
2/5
20
I N D U S T R I A L
A N D
E N G I N E E R I N G C H E M I S T R Y Vol.
45,
No.
t
100
8
6
4
3
2
0
8
6
4
3
2
B u r k e
8a P l u m
__
R e
- E
Figure
1 .
Fric t ion
Factors
for Single-phase
Flow through
Packed Beds
7 4 )
In a second article Ergun
( 1 4 )
attempted to correlate data on
mass transfer from irregular shapes of packing pieces into liquid
or gaseous streams flowing through the equipment. Following
Osborne Reynolds' suggestion that the coefficients a and
a ,
s
well as
b
and b , be taken proportional to each other in
R = au u2
(2 )
( 3 )
for
the fluid resistance, R, and the mass transfer rate,
w,
as
a
function of fluid velocity, u, nd driving force,
AC,
Ergun con-
cluded tha t a new mass transfer factor, J , should be defined by an
equation equivalent to
w
= a AC +
b
p
u
AC
J
B e ( p c / p D , ) ( k ~ P / G ~ i ) 4)
Assuming th at th e factor of proportionality between a and a "
is the same as that between
b
and
b ,
Ergun concluded too that
J f k ( 5 )
with
fk
being given by Equation 1. Although this equation was
moderately successful
for
the correlation of data on mass trans-
fer
in
solid-liquid systems, the friction factor was 5 to
100
times
greater than
J
for solid-gas sys te m. This reviewer believes
th at this large discrepancy may be due more to the inadequacy of
the theory than to experimental errors in the various sets of
literature data.
Even for a shape as simple as a cylinder mounted
transverse to the fluid stream the form drag (excess fluid pres-
sure on the front face, caused by detachment of the boundary
layer) forms
a
large pa rt of the total frictional drag but contrib-
utes nothing t o mass transfer,
It
seems quite improper to as-
sume that b is the same fraction of
b
as
a
is of a; to do so neg-
lects the fact t ha t the frictional effect of changes in fluid direc-
tion for flow through tortuous channels causes more pressure drop
tha n it does mass transfer.
A
somewhat similar comparison of fluid friction and mas
transfer in packed columns was reported by Ranz
(SO),
mh
showed that drag coefficients and mass transfer coefficients fo
single, isolated spheres could be used to estimate the pressur
drop and mass transfer coefficients for beds of spheres throug
which gases flow. In each case the superficial fluid velocity ha
to be multiplied by a factor of about
10
in order to arrive at t h
right individual drag coefficient or a single-sphere mass-transfe
coefficient. Th at the factor was nearly the same for friction an
for mass transfer indicates tha t the form-drag effect is not greatl
different around single spheres and in beds
of
spheres.
Pratt
WQ)
reviewed existing data on absorption, vaporiza
tion, and distillation for packed columns and concluded that th
gas phase mass-transfer coefficients could be expressed by a
equation suggested by friction a nd mass transfer effects in wetted
wall columns
The value of
i c ~
s based on the tota l exposed surface
of
the pack
ing; the equivalent diameter, Deq , is defined as four times th
free space divided by the periphery
of
the packing;
L
in cubi
feet per hour per foot is based on th e same periphery, and is ca
culated by dividing the superficial liquid mass velocity (mass pe
unit t ime per unit area) by the product of th e liquid density an
the periphery in feet per square foot of column cross section
For random packings the to tal packing perimeter per square foo
of
column cross section is assumed equal to the exposed packin
surface per unit of packed volume.
The factor,
tu,
is represented graphically
in
the paper and in
creases roughly linearly from zero
t o
unity
as
the liquid rate in
creases from zero to th e minimum effective liquid ra te for max
mum wetting of the packing
(M.E.L.R.).
The 1LI.E.L.R. is
7/26/2019 Industrial & Engineering Chemistry Volume 45 Issue 1 1953 Pigford, R. L. -- Absorption and Humidification
3/5
January 1953 I N D U S T R I A L A N D
E N G I N E E R I N G C H E M I S T R Y
21
*
characteristic of the system, as indicated in Table I ;
a
and
vary with the packing, as shown in Table 11.
Differences in the M.E.L.R. in different liquid-gas systems
were suggested to be related to the heat of absorption of the
solute gas, possibly because the heat released a t th e interface and
th e resulting influence on interfacial properties may have affected
the tendency of t he liquid to sp read over the packing.
Table
1
Va l u e s o f M i n i mu m E f fec t i v e L i q u i d R a te f o r Ma x i mu m
W e t t i n g o f Pa c k in g
or
W e t te d - W a l l C o l u mn Ac c o r d i n g t o P ra tt 29)
Liquid System
M.E.L.R.,
Cu. Ft./(Hr.) (Ft.)
Wate r Vaoorization of water 0.7a
Wate r Abiorption of ethyl alcohol
1.0
Wate r Absorption of ammonia 1 . 7
Kerosene Absorption of organic vapors
< O
.26
Distillation 0.6-0.7
?c
a For regular packings with good distribution this may be as low as
0.4 cu. ft./(hr.)lft.)
Table
II.
Constants in Equatio n 6 Recomm ended by Prat t 29)
Packing
Type Size, inches Mode of installation
eoa
Drip-point grids No. 6897 Continuous flue 0.032 0.146
Drip- oint grids No. 6295 Continuous or crossed flue 0 .067 0.0 61
W?o$grids
7/g X
4
X 1/4
Continuous
or
crossed
flue
0.152
0
Triple spiral tiles
3
Continuous flue >0.034 0.068
Triple spiral t les
3
Staggered flue 0.046 0.120
Single s iral trles Stag ered flue 0.048 0.038
Berl saJdies 0. 5
to
1.5 Ranjom 0.072 0
Rasehig ring8 0,3 75 o 2 Random 0.123 0
Sherwood an d Holloway
(989,
from observed total resistance.
a Based on subt rac tio n of liquid film resistance, est imated from da ta of
The question of wetted and effective areas of packing was fur-
ther investigated by Shulman and DeGouff 34)who employed
a
new and clever experimental technique. They studied vaporiza-
tion of Raschig rings cas t from naphthalene into air with water
flowing through th e packing. Since the naphthalene was in-
soluble in water, vaporization into the a ir occurred only from the
portions of th e packing th at were dry. Measurements of rates of
absorption of carbon dioxide from water agreed closely with pre-
vious, generally accepted data, showing that the liquid distri-
bution was satisfactory. Rates of naphthalene vaporization with
the packing completely dry agreed very closely with the data of
Taecker and Hougen
36)
or vaporization of water, af ter a cor-
rection had been applied by assuming
k~
proportional to
DyZ/*.
By
measuring the reduction in naphthalene vaporization rate
when the packing
was
irrigated the fraction of total packing sur-
face area that was wetted could be calculated, leading to the re-
sults shown in Figure 2.
by the gas flow rat e and by th e liquid %ow rate. The dips in the
curves are more pronounced a t th e lowest liquid rate, suggesting
that the minimum is caused by the
fac t
th at the liquid layer
on
the packing is thin enough for the gas to blow it
o f f
easily. The
gas-liquid interfacial area t ha t is effective in countercurrent trans-
fer processes is generally greater tha n the wetted packing area, as
Shulman and DeGouff 34) ound when they compared their cor-
rected naphthalene vaporization rate coefficients with Fellingers
(16)
oefficients for ammonia absorption (corrected for liquid-
film resistance). Presumably the drops and spray surface formed
inside the packing are responsible for the excess of gas-liquid in-
terfacial area over liquid-solid interface, the ratio
of
the two being
as large as 1.4 n some circumstances.
Procedures for the design of commercial gas absorbers in which
gas-film resistance predominates were reviewed by Williamson
39). New data were reported on the effect of different kinds of
liquid distributors on packing performance and on liquid entrain-
ment. Table I11 shows the variation of performance of a tower
filled with 3-inch rings stacked 8 feet deep at L
=
2200 pounds
per hour per square foot and a t a gas velocity
of 4
feet per second.
As may be seen in the figure, the wetted area is influenced both
Tab le
Ill.
E f fe c t o f M e t h o d of L i q u i d D i s t r i b u t i o n
on
Relat ive
Packing Performance 39)
Relative
Packing
Type
of
Distributor Performance
Trough distributor,
1
inch wide troughs evenly spaced a t 4.5
inches 100
Vertical pipe discharging downward o nto packing, qne distribu-
tion point per 2.25 square fee t of tower cross section 16
Vertical pi e disoharging downward
9
inches above flat target
p la te l a 8
on
packing, one distribution point per 2.25 square
feet
of
tower cross section 76
Vertical pipe discharging dortnward above 18 inches deep layer
Outlet 9 inches above packing, one distribution point per
Outlet a t top level of packing, one distribution p oint per 2.25
Outlet 6 inches above packing, one. distribution point per
of random packing
2.25 square fee t of tower cross section
square fe et of tower cross seotion
0.56 square foot of tower cross section
63
5 9
120
~~
The tower was used to cool water by evaporation into air, and
85
to
90 of
the total mass transfer resistance was estimated
t o
be
in the gas phase.
Liquid entrainment was found to be less than 0.1 pound per
1000 pounds of air with 2-inch serrated wood-grid packing and
was considerably greater with 3-inch random ring packing. With
the latter, a trough-type distributor gave much less entrainment
than a splash-type distributor made from a pipe discharging onto
the top of the packing.
Mass and heat transfer in a 6-inch square tower filled with 1 X
l/*-inch carbon grids was studied extensively by Norman M)
who reported over-all coefficients for ammonia absorpt ion in
water and for evaporative cooling of water. The results were
ex-
pressed by the formula
(7)
O G=
p(G/lOOO)O.*
feet
0, or HOG t
G
= 1000 f t .
L,
lb./(hr.)(sq.
f t . )
Water cooling
NH3
absorption
930
1400
1640
1870
2100-2810
2900
1.88
. . .
1.57
1.53
. . .
The carbon grid packing was found to be more efficient than
the common 1-inch ring packing as indicated b y t he following com-
parison based on operation a t L / G
=
1.
Pressure Drop,
Inch
HzO
Capacity
G
= L ,
Per Figure
of
lb./ hr.) HOG, Transfer Merit,
Packing (sq.
f t . )
f t . Unit G I H o Q
Carbon grid
2500 1.75
0.19 1430
1-Inch rings
500 1 . 6 0 .48 310
The grid packing can be used at a higher gas velocity without
flooding and without a large friction
loss.
The high allowable
velocity and small height of a transfer unit results in
a
compara-
tively small packed volume for scrubbing a given quantity of gas.
Norman (86) lso studied the spreading flow of water an d
kerosene over a grid element, introducing the liquid a t a single
point on the top edge of the element. Glass, stoneware, and
bright metal surfaces could be wetted uniformly when they were
perfectly clean, but the slightest contamination caused the film
to break down. Wood and rusted iron surfaces were easily
wetted b ut slight surface irregularities interfered with t he liquid
flow an d made it difficult to obtain reproducible results. Finally
it was found th at certain types of carbon provided an ideal
sur-
face which could be wetted uniformly without the need for clean-
ing, and gave reproducible results even after considerable han-
dling and exposure to the atmosphere. The water films spread
1-Inch rings 700 1 .6 0.96 435
7/26/2019 Industrial & Engineering Chemistry Volume 45 Issue 1 1953 Pigford, R. L. -- Absorption and Humidification
4/5
22 I N D U S T R I A L A N D E N G I N E E R I N G C H E M I S T R Y Vol. 45, No.
L
IO
G GAS RATE LB./ HR.) SQ.FT,)
Figure 2.
Effect of
Gas
R at e on W et t ed A rea of Packed Gas
Absorber
3 4 )
more rapidly and completely when the liquid rate was high and
when the liquid stream was allowed to fall
0.25
or 0.50 inch ont o
the top edge of t he packing tha n when it did not fall freely a t all.
Water and kerosene behaved alike.
Table IV. Constants in Dal l -and-Prat t Equat ion for Flooding
V e l o c i t y
Values of Dimensionless Constants,
C2
and
p
M > iMorit io s1
< M o ri t i a a l
___-
Type of Packing cz
P
Mcritiosl Cz
P
Random Raschig rings
0.64 -0 .20
0 . 4 7 0 . 3 3 - 0 . 3 6
Stacked Raechig rings , , , 0 . 7 2 - 0 . 3 6
Random Berl saddles 0.69
- 0 2 0
0 . 2 5
0 .42
- 0 . 3 6
Random wire helices . . . , , 0 .24 -0 .44
Extensive and accurate data on mass and heat, transfer coef-
ficients for air-wat-r contact in a 21.5-inch square tower filled
wiCh 1.5-inch Berl saddles were reported b y Hensel and Treybal
(20). Some of their conclusions were similar to those reached
earlier by McAdams, Pohlenz, as d St. John
34):
the psychro-
metric ratio was generally higher than the humid heat, probably
because the effective area for hea t transfer was as much as twice
th at for mass transfer; and the dynamic equilibrium temperature
of t he recirculated water was sometimes as much as
6' F.
above
the adiabatic saturation temperature of the entering air. The
transfer coefficients increased very rapidly with increasing gas
velocity as the loading point was reached.
A
comprehensive review of existing data on flooding velocities
in packed columns was made by Dell and Pratt ( 1 2 ) along lines
suggested by Bert etti 7 )and by their own earlier paper on flood-
ing phenomena for two-phase liquid-liquid flow in packed ex-
tractors
( I S ) .
Based on the idea that the frictional effects re-
sponsible for flooding are friction of the gas and liquid against the
packing and not against each other, the following equation was
found to correlate several sets of publ ished da ta for packing
larger than 0.25 inch, except for 0.50-inch packings when use
with very viscous liquids.
1
+ M
= C2Y
(8
where A
=
~ G / ~ L ) ~ ~ ~ ~ ~ L / ~ C L , ) ~ . ~ ~
/G)0.64
1 =
vGza/gLea)(PG/PLj(a~Q/8Q
The authors point out that the values
of
CZ
Table
I V )
vary
from one packing to another in t he same direction as the variation
of fluid friction for these packings; flow through stacked ring
occurs with the lowest pressure drop, followed in turn by Ber
saddles and random rings.
The change in
p
a t a critical value of
M
is thought to be associated with
a
transition in t he type qf flow i
one phase.
Measurements of liquid and gas-phase resist
ances on small bubble trays have been described previously by
Gerster, Colburn, Bonnet, and Carmody
(29).
These measure
ments have now been extended by Gerster, Bonnet, and Hess 18
who have shown th at the resistance in each phase is affected by
the dens ity of the foam and by the liquid time of contact as i
flows
across th e tray . Tests of oxygen stripping efficiencies on
large tray section having
a
liquid f l o ~ ath about 5 feet lon
were found to agree with an extrapolation of similar data from
small-tray measurements.
When the long tray was operated a
high horizontal liquid velocities, causing a variation in liquid
depth and a nonuniform distribution of air flow through the dif
ferent caps, the liquid-film resistance was increased, apparently
because only
a
few
of
th e caps were bubbling.
Tray
Towers.
A I R OUT
I
WATER IN
-
-
,
,,
AS-TO-LIQUIDURFAC: ~
HEAT EXCHANGER
COOLING
TOWER
-
WATER OUT
Figure 3 . Use of Au xi l iar eat Exchanger to Produce Water
Colder than
Air k ?-Bulb
Temperature (7)
New data on foam densities and point cJfficiencies
for
air-wate
contact on perforated trays weie published by West, Gilbert , and
Shimizu
(58).
The gas-phase resistance was determined by th
wet-bulb humidification of air and the liquid-phase resistance by
absorption and desorption of carbon dioxide. Th e correlation o
the data w s attempted by a method similar to that proposed by
Geddes
(179,
based on the assumption of transient diffusion
through stagnan t liquid and gas near the interface
of
a completel
formed bubble. (The mass transfer during the period of bubble
formation was not included. The theory requirm value of the
time of contact between gas and liquid, which was taken a s the
time required for the bubble to rise a distance eqLal to its diam
eter, thus assuming that the liquid at the interface is contin-
uously replaced from the stagnant
pool
where th e bubble enter$
The effective bubble diameter that should be used with the
theory to account for the observed tr ay efficiencies was computed
using observed values of foam density
to
estimate contact time
7/26/2019 Industrial & Engineering Chemistry Volume 45 Issue 1 1953 Pigford, R. L. -- Absorption and Humidification
5/5
January 1953 I N D U S T R I A L A N D E N G I N E E R I N G C H E M I S T R Y 2
The resulting values range from about 0.33 to 0.55 inch for ab-
sorption, desorption, and humidification and a re roughly inde-
pendent of the gas and liquid rates and the initial liquid depth.
The average value of 0.50 inch agreed very closely with equivalent
bubble diameters calculated by West
t al. (88)
rom the data of
Gerster, Colburn, Bonnet, and Carmody (19) or bubble-cap
plates, These equivalent diameters were larger tha n the center-
to-center distance between adjacent holes in the perforated tray .
Using these bubble diameters without correction
for
physical
properties, bubble-tray efficiencies were predicted for methanol-
water rectification and for furfural extractive distillat ion of bu-
tane-butene with disappointing results. The predicted efficiencies
Cross and Ryder
( 1 1 )
found
that
the formation of gas bubbles
at submerged orifices is strongly affected by l iquid surface tension
when the gas rate is low. Thus, th e depression of the gas-liquid
interface below the tops
of
the slots of a bubble cap cannot be
calculated from the hydrodynamic weir formula alone, as was
suggested by Rogers and Thiele
(3 )
n 1934. Below a critical
gas flow rate, th e slot opening is nearly constant a nd independent
of the gas flow. For water this critical opening ranges from about
2
inches for very narrow slots (ca. 0.01 inch +$e)
to
about 0.20
inch for
slots
wider than abou t an inch.
were substantially different from those of Gerster
et
al. f8).
II
ABSORPTION PROCESSES
Commercial practices in the removal of carbon dioxide and
carbon monoxide from coke oven gas and natural gas by absorp-
tion were described by Yeandle and Klein
( 4 1 ) .
Carbon dioxide
is removed by scrubbing the gas with a n amine solution or with
water under pressure and carbon monoxide is taken out with
copper ammonium formate or acetate. A unique process for
removing carbon monoxide, methane, argon and acetylene
from hydrogen was also described.
It
involves scrubbing the
hydrogen-rich gas with liquid nitrogen from an ai r liquefaction
plant, followed by flashing a part of the liquid effluent to purge
th e system of th e dissolved gases.
Severe corrosion of carbon-steel tubes of a reboiler handling a
30 volume yoaqueous solution of monoet,hanolamine containing
small amounts of dissolved carbon dioxide and hydrogen sulfide was
reported (9). The boiling solution was heated by oil
at
500
F.
If this temperature was reduced to 370 F. or if hydrogen sulfide
was absen t th e corrosion was very much reduced. Th e discussion
of
this paper brought out t ha t corrosion is generally less severe in
absorption plants using both ethylene glycol and ethanolamine,
even though t he boiling point of these solutions is higher than tha t
of the
aqueous solution of ethanolamine alone.
COOLING TOWERS
A novel method of using a cooling tower in conjunction with
auxiliary surface-type heat exchangers t o produce cold water
at
a
temperature lower than t he wetrbulb temperatu re of th e evail-
able air was described b y Agnon and Young
1 ) .
I n
its
simplest
air by transferring heat t o cool the water, which is then recycled
to the tower,
as
shown by Figure
3.
In a
typical example, proc-
ess water was cooled from 78 to 67
F.
using air having a wet-
bulb temperature of
69
F. (which was reduced to
62
F. in the
air
cooler). The quanti ty of water circulated through the cooling
tower was 2.5 times the ra te of supply of fresh water. In
an
ex-
tension of the same idea, the cool, saturated air leaving the cool-
ing tower can be used to cool the fresh air, and in the same ex-
ample,
the
water flow through the tower would be reduced in thi s
method of operation to
1.43
times the water feed rate.
6
version their process employs a hea t exchanger for precooling th e
NOMENCLATURE
a
D ,
= specifie surface of d ry packing, square feet per cubic foot
= diameter of
a
sphere having the same ratio of surface to
of packed volume
volume
as
a piece of packing, feet
go =
standard gravitational conversion factor, (lb. mass)(ft.)
=
local gravitational acceleration,
f t . b . 2
? =
superficial mass velocity of gas, lb./(hr.)(sq . it .)
HOG heigh t of an over-all gas-film transfer unit, feet
L =
superficial
mass
velocity of liquid, lb./(hr.)(sq. ft.)
N R ~
D,G/p
=
Reynolds number for flow through packed be
VQ
= superficial velocity
of gas, feet
per hour
U =
superficial velocity, fe et per hour
Z =
depth of bed, feet
e
= fraction free space in d ry packing
jw
=
viscosity
of
gas, lb./(ft.)(hr.)
p~ =
viscosity of liquid, lb./(ft.)(hr.)
p
=
fluid density lb./cu.
f t .
PQ
=
gas density ib. cu. f t .
p~
=
liquid density, i ./cu.
f t .
(Ib. force)(hr.Z)
REFERENCES
1)
Agnon,
S.,
and Young, ChiaYung,
Heating, Piping A ~ To n d
(2) Amick, E. H.,
Jr.,
Johnson, W.
B.,
and Dodge, B.
F.,
Chem
(3) Arnold, J. H., Ibid.,
No.
3, 82-92 (1952).
(4) Baldwin, R. R., and Daniel, 6. G., J. AppZ. Chem.,
2 ,
161-
(5)
Benedict, M., Webb, G. B.,
and
Rubin,
L
C.,
J. Chem. Phys
8 ,
334 (1940); 10, 747 (1942); Chem. E w . Progr., 47, 419
(6) Benedict, M., Webb, G. B., Rubin, L. C., and Friend, Leo
Chem. Eng Progr., 47, 571-8, 609-20
(December
1951).
(7)
Bertetti,
J.
W.,
Trans. Am. I nst. Chem. Engrs.,
38, 1023 (1942
8)
Burke,
S.
P., and Plummer, W. B.,
IND.
NG.CHEM.,
0, 119
(9)
Carlson, E.
C.,
Davis, G. R., and Hujsak, K.
L., Chem. Eng
tioning,
24,
139-42 (October 1952).
Eng. Progr., Symposium Ser., 48, 65-72 (1952).
(April 1952).
449-54 (1951).
(1928).
Progr., 48, 333-6 (1952).
(10) Carman, P.
C.,
Trans.Jnst. Chem. Engrs., 15, 150 (1937).
(11)
Cross,
C. A., and Ryder,
H.,
J . AppZ. Chem., 2, 51-60 (Febru
(12) Dell,
F.
R., and Pratt, H. R. C., Ibid., 2,429-35 (August 1952
(13)
Dell,
F.
R.
and Pratt,
H.
R. C.,
Trans. Inst. Chem. Engrs.,
29
(14)
Ergun,
S., Chem. Eng. Progr., 48, 227-36 (1952).
(15) Ergun, S., and Orning,
A.
A.,
IND.
NG.CHEM., 1,1179 (1949
(16) Fellinger, L. L., Sc.D. thesis, Mass. Inst. Technol., 1941.
(17)
Geddes,
R.
L.,
Trans. Am. Inst. Chem. Engrs., 42, 79 (1946).
(18)
Gerster,
J .
A., Bonnet, W. E., and Hess,
I.
Chem.
Eng. Progr
(19)
Gerster,
J.
A., Colburn, A. P., Bonnet, W. E., and Carmody
(20)
Hensel, S., and Treybal, R. E.,
IbicE.,
48,
362-9 (1952).
(21) Hughes,
H.
E., and Maloney,
J.
O.,
Ibid.,
48, 192-200 (1952)
(22)
Kirkbride,
C.
G., and Bertetti, J. W.,
IND.
NG. CHEM.,
5
ary
1952).
89 (1951).
47, 223-7, 621-7 (December 1952).
T.
W.,
Ibid., 45, 716-24 (1949).
1242 (1943).
(23) Kozeny, J.. Sitzber. Akad. Wiss Wien. Math.-naturw. Klass
Abt. IIa , 136, 271 (1927).
Eng. Prop., 45, 241 (1949).
(24) McAdams, W. H., Pohlenz,
J.
B., and St. John,
R.
C., Chem
(25)
Norman, W.
S., Trans.
Inst.
Chem. Engrs.,
26,
81 (1948).
(26) Ibid.,
29,
226-39 (1951).
(27) Organick,
E.
I., and Brown,
G.
G., Chem. Eng. Progr., Sym
(28)
Plewes,
A.
C., and Klsssen,
J., Can. J . Technol., 29, 322-3
(29) Pratt,
H.
R. C., Trans. Inst. Chem. Engrs.,
29,
195-214 (1951
(30) Ranz, W. E., Chem. Eng. Proor., 48, 247-53 (1952).
(31) Ranz, W. E., and Marshall, W. R., Jr., Ibid., 48, 141-6, 173-8
(32)
Rogers,
M.
C., and Thiele, E. W.,
IND.
NG. CHEM.,
26, 82
posium
Ser., No. 2 ,
48, 97 (1952).
(July 1951).
1952).
(1934).
(33) Shkrwodd,
T.
K., and Holloway,
F.
A. L., Trans. Am.
Ins
(34)
Shulman, H. L., and DeGouff.
J. J..
Jr..
IND.
NG.CHEM..
4
Chem. Engrs., 36, 39 (1940).
.
1915-22 (1952).
93-8 (1952).
1949).
(1940).
(35) Solomon, E., Chem. E w . Prog., Symposium Ser., No. 3, 48
(36) Taecker, R. G., and Hougen, 0. A.,
Chem.
Eng. Progr., 45, 18
(37) Webber, C.
E.,
Am. Inst. Mining Met. Engrs., Tech. Pub.
125
(38)
West,
F. B.,
Gilbert,
W.
D., and Shimizu,
T.,
IND. NG.CHEM
(39) Williamson, G. f . , Trans.
Ins t .
Chem. Engrs.,
29,
215-25 (1951
(40)
Winn, F. W.,
Chem. Eng. Progr., Symposium Ser., 48, 121-3
44, 2470-8 (1952).
(1952).
---- -
(41) Yeandle, Wd W., and Klein,
(3. F.
Chem. Eng. Progr., 48, 344
52 (1952).