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14-68 EQUIPMENT FOR DISTILLATION, GAS ABSORPTION, PHASE DISPERSION, AND PHASE SEPARATION<br />
11 of Kister’s Distillation Design (McGraw-Hill, New York, 1992)<br />
leads to a similar conclusion for structured packings. For water-rich<br />
systems, packing HETPs tend to be much higher than for nonaqueous<br />
systems due to their high lambda or surface underwetting, as discussed<br />
above. High hydrogen concentrations (>30 percent or so in the<br />
gas) have also led to low packing efficiencies (Kister et al., Proc. 4th<br />
Ethylene Producers Conference, AIChE, New Orleans, La., p. 283,<br />
1992), possibly due to the fast-moving hydrogen molecule dragging<br />
heavier molecules with it as it diffuses from a liquid film into the<br />
vapor.<br />
Errors in VLE These affect packing HETP in the same way as<br />
they affect tray efficiency. The discussions and derivation earlier in<br />
this subsection apply equally to tray and packed towers.<br />
Comparison of Various Packing Efficiencies for Absorption<br />
and Stripping In past editions of this handbook, extensive data on<br />
absorption/stripping systems were given. Emphasis was given to the<br />
following systems:<br />
Ammonia-air-water Liquid and gas phases contributing; chemical<br />
reaction contributing<br />
Air-water Gas phase controlling<br />
Sulfur dioxide-air-water Liquid and gas phase controlling<br />
Carbon dioxide-air-water Liquid phase controlling<br />
The reader may refer to the data in the 5th edition. For the current<br />
work, emphasis will be given to one absorption system, carbon dioxide-air-caustic.<br />
Carbon Dioxide-Air-Caustic System The vendors of packings<br />
have adopted this system as a “standard” for comparing the performance<br />
of different packing types and sizes for absorption/stripping.<br />
For tests, air containing 1.0 mol % CO2 is passed countercurrently to<br />
a circulating stream of sodium hydroxide solution. The initial concentration<br />
of NaOH in water is 1.0 N (4.0 wt %), and as the circulating<br />
NaOH is converted to sodium carbonate it is necessary to make a<br />
mass-transfer correction because of reduced mass-transfer rate in the<br />
liquid phase. The procedure has been described by Eckert et al. [Ind.<br />
Eng. Chem., 59(2), 41 (1967); Chem. Eng. Progr., 54(1), 790 (1958)].<br />
An overall coefficient is measured using gas-phase (CO2) concentrations:<br />
moles CO2 absorbed<br />
KOGae = ������<br />
time-bed volume-partial pressure CO2 driving force<br />
(14-161)<br />
The coefficients are usually corrected to a hydroxide conversion of 25<br />
percent at 24°C. For other conversions, Fig. 14-14 may be used.<br />
Reported values of KOGa for representative random packings are given<br />
in Table 14-15. The effect of liquid rate on the coefficient is shown in<br />
Fig. 14-63.<br />
While the carbon dioxide/caustic test method has become accepted,<br />
one should use the results with caution. The chemical reaction masks<br />
TABLE 14-15 Overall Coefficients for Representative Packings<br />
CO2-air-caustic system<br />
Nominal size,<br />
mm<br />
Overall coefficient KOGa, kg⋅moles/(hr⋅m3⋅atm) Ceramic raschig rings 25 37.0<br />
50 26.1<br />
Ceramic Intalox saddles 25 45.1<br />
50 30.1<br />
Metal pall rings 25 49.6<br />
50 34.9<br />
Metal Intalox saddles (IMTP ® ) 25 54.8<br />
50 39.1<br />
NOTE: Basis for reported values: CO2 concentration in inlet gas, 1.0 vol %; 1N<br />
NaOH solution in water, 25 percent NaOH conversion; temperature = 24°C;<br />
atmospheric pressure: gas rate = 1.264 kg/(s⋅m2 ); liquid rate = 6.78 kg/(s⋅m2 ).<br />
SOURCE: Strigle, R. L., <strong>Packed</strong> Tower Design and Applications, 2d ed., Gulf<br />
Publ. Co., Houston, 1994.<br />
K Ga, lb-moles/hr, ft 3 , atm<br />
K Ga, lb-moles/hr, ft 3 , atm<br />
10<br />
5<br />
3<br />
2<br />
1<br />
.8<br />
.6<br />
.4<br />
.3<br />
.2<br />
0.1<br />
100 500 1000 2000 5000<br />
2<br />
Liquid rate, lbm/(hr•ft )<br />
(a)<br />
10<br />
5<br />
3<br />
2<br />
1<br />
.8<br />
.6<br />
.4<br />
.3<br />
.2<br />
0.1 100<br />
1<br />
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p<br />
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1<br />
2<br />
a<br />
r<br />
'<br />
'<br />
the effect of physical absorption, and the relative values in the table<br />
may not hold for other cases, where much of the resistance to mass<br />
transfer is in the gas phase. Background on this combination of physical<br />
and chemical absorption may be found earlier in the present section,<br />
under “Absorption with Chemical Reaction.”<br />
l<br />
l<br />
n<br />
i<br />
r<br />
a<br />
a<br />
r<br />
s<br />
'<br />
'<br />
2<br />
s<br />
c<br />
c<br />
g<br />
i<br />
h<br />
p<br />
h<br />
s<br />
l<br />
a<br />
g<br />
i<br />
g<br />
l<br />
r<br />
r<br />
i<br />
r<br />
i<br />
n<br />
i<br />
n<br />
n<br />
g<br />
g<br />
g<br />
s<br />
500 1000 2000 5000<br />
2<br />
Liquid rate, lbm/(hr•ft )<br />
FIG. 14-63 Overall mass transfer coefficients for carbon dioxide absorbed<br />
from air by 1N caustic solution. (a) 1-in Pall rings and Raschig rings. (b) 2-in Pall<br />
rings and Raschig rings. Air rate = 0.61 kg/s⋅m 2 (450 lb/hr⋅ft 2 ). To convert from<br />
lb/hr⋅ft 2 to kg/s⋅m 2 , multiply by 0.00136. To convert from lb-moles/hr⋅ft 3 atm to<br />
kg-moles/s⋅m 3 atm, multiply by 0.0045. [Eckert et al., Chem. Eng. Progr., 54(1),<br />
70 (1958).]<br />
(b)<br />
s<br />
s