Ind. Eng. Chem. Process Des. Dev. 1981, 20, 540-545
540
It is desirable industrially to carry out hydrodenitrogenation with as little consumption of hydrogen as possible. Saturation of the N-containing ring and subsequent hydrocracking to propyl benzene and NH3 represents the absolute minimum on present-day catalysts. In fact, however, most of the hydrocarbon product is saturated. Table I shows the effect of presence of water vapor and/or H2S on the PCH/PBz ratio at 375 "C and at 420 "C, for selected % conversions at which comparisons could be made. At 375 "C, the ratio is slightly increased by water vapor alone but is markedly increased by H2S. A mixture of H2S and H20 vapor behaves like H2S alone. Although H2Saccelerates the overall HDN rate, it is seen that in its presence the hydrocarbon product is on average more highly saturated. A t 420 "C the PCH/PBz ratio is decreased below that at 375 "C for each case. H2S slightly increases the ratio and water vapor slightly reduces it. Although water vapor reduces the HDN rate at 420 "C, in its presence the hydrocarbon product is on average less highly saturated. The only other study of the effect of water vapor on HDN of a heterocyclic nitrogen compound of which we are aware is a brief report in the thesis of Goudriaan (1974) of the HDN of pyridine over a CoMo catalyst in either the "oxidic" form or in the presence of H2S. With the oxidic catalyst at 250 "C water vapor caused a marked decrease in ring hydrogenation activity (rate of formation of piperidine), but the rate of hydrogenolysis was too low to observe an effect of water vapor. With the sulfided catalyst at 300 "C and in the presence of 2 bar (200 P a ) H a , water vapor did not affect ring hydrogenation activity. Hydrogenolysis activity was likewise not affected by water vapor up to 1 bar (100 kPa) but' was enhanced at higher water vapor pressures. Literature Cited
Table I. Effects of Water Vapor and Hydrogen Sulfide on Ratio of Propyl Cyclohexane t o Propyl Benzenea quinoline quinoline quinoline quinoline + H,O alone + H,O + H,S andH,S
3 7 5 " C , 23% HDN 3 7 5 'C, 47% HDN 420"C, 50% HDN 4 2 0 OC, 94% HDN
5.4
6.4
17
18
4.2
5.7
19
19
3.1
2.3
4.1
3.0
2.7
3.5
--
a P = 7 MPa;p.p.g= 1 3 . 3 kPa;p.p.H,o= 1 3 . 3 kPa; p . p . ~ , 1~3=. 3 kPa.
A comparison of the rate constants in the presence of water at 375 "C to those in its absence (Satterfield and Cocchetto, 1980) yielded the following results R1 = 0.000164/0.00020 = 0.82
R2 = 0.0044/0.0052 = 0.84 R3
= 0.0185/0.0238 = 0.78
R4 = 0.0020/0.00172 = 1.16 R, = 0.0013/0.00133 = 0.98 where
Ri =
(ki)~HW=13.3 E a
(ki)P~=o.o
and the subscript i refers to the reaction as noted in Figure 4. Water vapor seems to have a moderate inhibiting effect on reactions 1and 2 but essentially none on reaction 7. It seems to affect the two hydrogenation reactions in opposite ways, accelerating 4 and inhibiting 3. However, the precision with which K4 can be determined is somewhat less than that for the other constants (Satterfield and Gultekin, 1981) so this may be an artifact of the model. None of the effects are major at this temperature and partial pressure, indicating that water vapor is not strongly adsorbed on a sulfided catalyst at these conditions. Overall, water vapor slightly enhanced the reaction path PyTHQ DHQ PCH in contrast to PyTHQ OPA PB, and consequently the ratio PCH/PB in the final products was moderately greater (Table I).
Carter, D. L. M.S. thesis, M.I.T., Cambridge, MA, 1980. Cocchetto, J. F.; Satterfleld, C. N. Ind. Eng. Chem. Process Des. Dev. 1981, 20, 49. Goudriaan, F. Thesis, Twente Universlty of Technology, Enschede, The Netherlands, 1974. Himmelbhu, P. M.; Jones, C. R.; Bischoff, K. B. Ind. fng. Chem. Fundem. 1987, 6, 539. Satterfbld, C. N.; Cocchetto, J. F. Ind. Eng. Chem. Process Des. Dev. 1981, 20, 53. Satterfiild, C. N.; Gbkekin, S. Ind. fng. Chem. Process Des. Dev. 1981, 20. 62. Satterfbld, C. N.; Modell, M.; Hies, R. A.; Declerck, C. J. Ind. fng. Chem. Process Des. Dev. 1978, 17, 141.
- - - -
Received for review August 25, 1980 Accepted April 6,1981
Heat Transfer Coefficient in Bubble Columns Haruo Hlktta,' Satoru Asal, Hlroshl Klkukawa, Toshlakl Zalke, and Masahlko Ohue Depament of Chemical Engineering, University of Osaka Prefecture, Sakai, Osaka 59 1, Japan
Experimental data on the heat transfer between the d u m n wall and the gas-liquid dispersions in the bubble column with a single nozzle gas sparger were obtained by using air and various liquids. A new dimensionless correlation for the heat transfer coefficient was presented and shown to correlate the experimental data with an average deviation at 3.9%.
Introduction Bubble columns are widely used in the chemical industry as absorbers, fermenters, and gas-liquid reactors. In order 0196-4305/81/1120-0540$01.25/0
to attain the required liquid temperature and its subsequent control, heat must be removed or supplied. Thus, information on heat transfer coefficients h, between the 0
1981 American Chemical Society
Ind. Eng. Chem. Process Des. Dev., Vol. 20, No. 3, 1981 541
cooling or heating surface and the gas-liquid dispersed bed is required in designing the bubble columns. Such heat transfer coefficients have been measured by numerous investigators (Kolbel et al., 1958, 1960; Fair et al., 1962; Kast, 1962,1963; Yoshitome et al., 1965; Ruckenstein and Smigelschi, 1965; Burkel, 1972; Hart, 1976; Nishikawa et al., 1977; Steiff and Weinspach, 1978) for various geometries of heating elements. However, most of the previous data were obtained at relatively low gas velocities and the effect of the physical properties of the gas and liquid on the heat transfer coefficient has not been studied very extensively. In the present work, the heat transfer coefficients from the wall of the bubble column provided with a single nozzle gas sparger were measured at relatively high gas velocities by using air and various liquids to clarify the effect of liquid physical properties, and a new dimensionless correlation for the heat transfer coefficient was presented. Previous Correlations Various empirical correlations for the heat transfer coefficient in the bubble columns have been proposed by a number of investigators (Kolbel et al., 1958,1960; Kast, 1962, 1963; Yoshitome et al., 1965; Burkel, 1972; Hart, 1976; Nishikawa et al., 1977; Steiff and Weinspach, 1978). A summary of the previous correlations was presented by Steiff and Weinspach (1978). Most of these correlations can be applied only a t low gas velocities and predict the modified Stanton number, hw/pcpuG,as functions of the product of the Reynolds number and the Froude number, uG3p/pg, and the Prandtl number, c # / k . Here, UG is the superficial gas velocity, p , p, cp, and k are the density, viscosity, specific heat, and thermal conductivity of the liquid, and g is the gravitational constant. Recently, Deckwer (1980) reviewed the literature and found that the Stanton numbers predicted from the various previous correlations did not differ much with each other. He also presented the following semitheoretical correlation
which was obtained by combining Higbie’s surface renewal model applied to heat transfer with Kolmogoroff s theory of isotropic turbulence. This equation almost completely corresponds to the correlation proposed by Kast (1962, 1963)and agrees well with the available experimental data obtained at low gas velocities. Nishikawa et al. (1977) measured the heat transfer coefficients in the bubble column over a wide range of the superficial gas velocities, using air and various liquids of different properties, and presented the following correlations for the Stanton numbers. For uG < 0.028 m/s
For uG > 0.028 m/s
(2b) where Ap is the density difference between the liquid and gas and pw is the liquid viscosity at the wall temperature. Equation 2a is not dimensionless and UG in the last term
-
2i: Figure 1. Schematic diagram of experimental apparatus: 1,blower; 2, rotameter; 3, gas inlet nozzle; 4, bubble column; 5, thermocouple; 6, heat transfer section; 7, slide rheostat; 8, voltage stabilizer.
10-cm 19-cm column column A : 20mm 50mm
B : 5mm 5mm C : 3 5 m m 65” D : 5 0 mm 120mm
Figure 2. Detail of heat transfer section: 1,flange (resin); 2, thermocouple; 3, packing (silicone rubber); 4, nichrome wire; 5, mica sheet; 6, brass ring; 7, asbestos.
of the right-hand side must be expressed in m/s. In the present work, the experimental results for the heat transfer coefficient were compared with the above two correlations. Experimental Section The schematic diagram of the experimental apparatus is shown in Figure 1. Two bubble columns were used. One of them was made of acrylic resin and was 10.0 cm i.d. and 162 cm in height. The other was constructed of transparent vinyl chloride resin and was 19.0 cm i.d. and 240 cm in height. The gas sparger used was of the single-nozzle type. For the 10-cm column two nozzles of 0.9 and 1.3 cm i.d. were used, while for the 19-cm column three nozzles of 1.31,2.06, and 3.62 cm i.d. were used. The nozzle was located 5 cm above the bottom plate of the column. Heat was supplied to the gas-liquid dispersion in the bubble column from the electrically heated heat transfer section. The heat transfer section, the detail of which is shown in Figure 2, was constructed of brass tube ring and w q inserted 105 cm and 80 cm or 160 cm above the bottom plate for the 10-cm column and 19-cm columns, respectively. The brass ring was wrapped with mica sheet to insulate it electrically from the heating element. The heating element was 1.0 mm or 2.0 mm diameter nichrome wire and was wrapped around the mica-covered brass section. This heating element was insulated with asbestos to reduce the heat loss into the surrounding air. The temperature at the surface of the brass section was measured by four and eight copper-constantan thermocouples of 0.2 mm diameter for the 10-cm and 19-cm columns, respectively, which were embedded at the middle of the brass section and were connected to the digital multi-thermometer (Yokogawa Electric Works Ltd., Type 2809). The temperature of the liquid in the column was measured by a copper-constantan thermocouple inserted in the central axis of the column at the same level as the
542
Ind. Eng. Chem. Process Des. Dev., Vol. 20, No. 3, 1981
Table I. Physical Properties of Liquids Used /1
liquid water
25.9 wt % sucrose
30.0 wt % sucrose
50.0 wt % sucrose
1-butanol 8.0 wt % methanol 15.0 wt % methanol 53.0 wt % methanol
x 103,
tL, "C
Pa s
20 25 30 35 20 25 30 35 20 25 30 35 20 25 30 35 35 20 25 20 25 15 20 25
1.01 0.894 0.803 0.719 3.11 2.67 2.28 1.94 3.86 3.28 2.77 2.38 17.1 13.1 10.0 8.11 2.00 1.26 1.07 1.46 1.26 2.00 1.71 1.46
P
x 10-3, kg/m3
cp x 10-3, J/kK
k, W/m K
x 103, J/m
4.18" 4-18" 4.18" 4.18" 3.18' 3.18' 3.22' 3.26' 3.01' 3.05' 3.09' 3.13 ' 2.39' 2.43 ' 2.46' 2.50' 2.71d 4.1gb 4.18b 4.16 4.15 3.51 3.55b 3.57b
0.594e 0.604e 0.614e 0.623e 0.516/ O.52lf 0.528/ 0.535/ O.50lf 0.508/ 0.514/ 0.519/ 0.437/ 0.443/ 0.449/ 0.453/ O.14gg 0.548h 0.555h 0.509; 0.515 0.331h 0.332h 0.333
72.8 71.8 71.0 70.2 74.1 72.0 71.4 70.8 74.3 72.0 71.5 70.8 75.5 74.0 72.0 71.5 23.9 58.1 58.0 52.5 52.5 38.5 38.2 37.8
0.998 0.997 0.996 0.994 1.12 1.12 1.12 1.12 1.14 1.14 1.14 1.13 1.23 1.23 1.23 1.23 0.802 0.990 0.985 0.976 0.974 0.913 0.912 0.910
a Perry and Chilton (1973, p 3-126). Perry and Chilton (1973, p 3-136). ' Huberlant (1959). (1970). e McAdams (1954). Riedel (1949). Reid et al. (1977). Riedel(1951).
middle of the heat transfer section, since the liquid temperature was uniform except very near the column wall. In most of the experimental runs the bubble columns were operated continuously with respect to the gas and batchwise with respect to the liquid, but in some runs the operation was continuous with respect to the liquid. The liquids used are given in Table I, together with their physical properties. Specific heats and thermal conductivities of the liquids were taken from the literature. Densities, viscosities, and surface tensions of the liquids were measured by means of conventional methods. The gas used was always air and it was fed from the nozzle to the bottom of the column after being metered with rotameters. The superficialgas velocity ue ranged from 0.053 to 0.34 m/s. The dispersed liquid height 2, was maintained at 145 cm and 170 or 230 cm for the 10-cm and 19-cm columns, respectively. The rate of heat transfer from the heated wall to the aerated liquid in the column was determined from the voltage and amperage readings by using Joule's law, taking the power factor as unity. The rate of accumulation of heat in the asbestos insulator was negligibly small after a definite operation time (about 30 to 60 min for 10-cm and 19-cm columns, respectively), as seen later, and the heat loss from the asbestos insulator into the surrounding air could be always neglected. The heat transfer coefficient h, was calculated by dividing the heat transfer rate by the heating surface area and the temperature difference between the heating surface and the bulk liquid, assuming quasi-steady-state conditions. The temperature difference was limited within about 3 to 10 "C to avoid the substantial variation of the physical properties of the liquid along the heat transfer path. Results and Discussion Experimental Data. Figure 3 presents the values of h, for the air-water system obtained at various liquid temperatures by operating the 10-cm column continuously in a countercurrent manner for the case of uL = 0.0034 m/s. It can be seen that the h, value is proportional to about the 0.15 power of the superficial gas velocity ue for each liquid temperature. The effect of the liquid flow rate
Riddick and Bunger
I
004
6
2
8 01
04
mls
UG ,
Figure 3. Heat transfer coefficient for water (continuous countercurrent operation). fL
20
20
25
30
*
'C 35 DT
= 1 0 cm
UG= ^ *
015 m/s
101
> 60
50
100
150
operation time , min
Figure 4. Comparison of heat transfer coefficient for water in semi-batch operation with that in continuous countercurrent operation.
on the h, value may be considered negligible in view of the previous work (Kast, 1962; Kolbel et al., 1958). Figure 4 shows the instantaneous values of h, measured at constant intervals of 5 min for the air-water system in the 10-cm column operated in a semi-batch manner for the case of U G = 0.15 m/s. In the semi-batch operation, the temperatures of the bulk liquid and the heating surface rise gradually with the elapse of time. In Figure 4 the h, values are shown as functions of the operation time and the bulk liquid temperature. A solid line represents the h, values for the continuous countercurrent operation which were estimated from the data shown in Figure 3. As can be seen in Figure 4, for the first 20 min after the start
20
I
I
Key dp.cm Z,.m
206
Z,,m
230
zOL
1.67
5 10-
Key Liquid D, cm o Water Water v 25.9% Sucrose 10 a 30.0% Sucrose 10 A 30.0% Sucrose 19 o 50.0% Sucrose 10
1:
-
I
0.04
2
8 0.1
6
Uo,
1,=25'C
0
-
,
0.4
)
/
I
m/s
Figure 6. Heat transfer coefficientfor water (semi-batchoperation): efecta of nozzle and column diameters, aerated liquid height and location of heat transfer section on h,.
,
20
I
I
I
I
'
1
10 -
1, ,'C
Liquid
\
-
8 % Methanol 15% Methanol 53% Methanol n-Butanol
35 20 20 20 35
lots!
1 10-2
2 61 4
-
3 4
5 6
I
2-
Present work Kat Hart Ruckenstem Smlgelschl Slelff-Wclmpch N18hiksWdet al F a r et al K 6 I M et al Vcshltane et al
-
8 9 10 Burke1
Wall
Wall Wall
--
_.
Wall Wall, Co~l Wall Coil Wall: Immd body Immd body Immd body COll
J
0.04
6
8 0.1 Ug
2
0.4
, m/s
Figure 8. Heat transfer coefficient for water, 1-butanol and aqueous methanol solutions.
It can be seen from this figure that the dependence of h, on uG for each sucrose solution is the same as that for water, and h, varies as 1 1 ~ O . l ~ .The h, value is seen to decreases with increasing concentration of sucrose. This decrease in h, may be mainly due to the increase in the viscosity of the sucrose solution, since the liquid properties other than viscosity did not change very greatly in the range of sucrose concentrations studied. In Figure 8 the h, values for water, pure 1-butanol, and aqueous methanol solutions in the 10-cm column are shown. The h,values for 1-butanol and aqueous methanol solutions were also found to vary as the 0.15 power of U G in the same manner as that for water. As can be seen in the figure, the values of h,for aqueous methanol solutions decrease with increasing concentration of methanol and the h, values for pure 1-butanol are considerably lower than those for water and methanol solutions. These results may be attributed to the combined effect of the surface tension, viscosity, and thermal conductivity of the liquid, since these liquid properties varied considerably in the present experimental runs. Correlation. As described above, the effects of the nozzle diameter do, the column diameter DT, the clear liquid height Z,, and the location of the heat transfer section Zh on the heat transfer coefficient h, can be neglected. Thus, the conceivable factors affecting h, are considered to be the superficial gas velocity uG,the liquid specific heat cp, the liquid thermal conductivity k, the
Ind. Eng. Chem. Process Des. Dev., Vol. 20, No. 3, 1981
544
0 041
4 0 -
B
-k 0
K
3
A
I
I
300% Sucrose
001
8
Key
6
v
3
v
4
A
m 0
0 002
Llquld Water 2599. Sucrose 300% SCrOW 500% Sucrose 8 0 % Methanol 150% Methanol 530% Methanol n-Butanol
I 1
4
6
8001
0.00
I
1
0 002
t .*/ 0 04
2
(hwlPcpuG)caI
Figure 9. Comparison of present data for Stanton number with proposed correlation.
liquid density p, the liquid viscosity p, the liquid surface tension u, and the gravitational constant g. In the previous work (Hikita et al., 1980,1981), the physical properties of the gas (density and/or viscosity) were found to affect appreciably the fractional gas holdup and the volumetric liquid-phase mass transfer coefficient. However, for the present problem the gas properties were not taken into account in obtaining the general correlation since they were anticipated to affect the flow pattern of the gas-liquid dispersion near the column wall indirectly. The dimensional analysis and the least-square method were applied to all the experimental data. The final correlation for the heat transfer coefficient h, is given by
assuming the exponent on the Prandtl number c,,p/k to be 2/3, which is generally recognized for forced convective heat transfer between the solid wall and the single-phase fluid flow. The ranges of the dimensionless numbers over which eq 3 is valid are as follows 5.4 x 10-4 < ( u G p / u ) < 7.6 x 4.9 7.7
X
10-2
< (cpp/k) < 93 < (p4g/p2) 1.6 X
lo*
Figure 9 shows the comparison of the observed and calculated values of the Stanton number h,/pcpuc. In this figure, the Stanton numbers observed in the present work are plotted on logarithmic coordinates against the Stanton numbers calculated from eq 3. The observed Stanton numbers are in good agreement with the calculated ones with an average deviation of 3.9% and a maximum deviation of 13.9%. In the previous work (Hikita et al., 1980, 1981), it was found that the aqueous methanol solutions give the unusual high values of the gas holdup and the volumetric liquid-phase mass transfer coefficient because of the coalescence hindering property of aqueous alcoholic solution. However, as can be seen from Figure 9, the measured values of h w / p C p U G for the aqueous methanol solutions can be well correlated by eq 3, indicating that the coalescence hindering property of the methanol solution does not affect appreciably the flow pattern of the
I/
Keys same as in Fig.9 I
4
6
8 0.01
2
i I 0.04
(hw~Pc,ut)cai
Figure 10. Comparison of present data for Stanton number with another correlation.
gas-liquid dispersion near the column wall. Equation 3 can be rewritten as hW = 0,411gO.308uG O.14Sc P0.333k0.667 P0.692 -0.286u-0.073 (4) I . 1 It can be seen from the above equation that the relation h, 0: u~0~149u-0~073 is valid. In our previous work (Hikita et al., 19801, it was found that the fractional gas holdup EG in bubble columns varies as the 0.578 power of UG and as the -0.158 power of u, i.e. 0: U G ~ . ~ ~ Therefore, U ~ . ~ . the relation h, 0: u~o'149U-0'073 obtained in the present work is in approximate agreement with the relationship h, 0: cG1/3 derived on the basis of the theoretical models proposed by Ruckenstein and Smigelschi (1965) and by Konsetov (1966). The above equation also shows that the heat transfer coefficient h, is not greatly affected by the liquid surface tension. If the effect of liquid surface tension on the h, value is ignored, we finally obtain the following correlation
Figure 10 compares the measured values of the Stanton number with those calculated from eq 5. Although the measured values of the Stanton number are in agreement with the calculated ones with an average deviation of 7.5% and a maximum deviation of 26.7%, the data points show the systematic error for the data of a few specified systems and display somewhat greater scattering than shown in Figure 9, indicating that the effect of the liquid surface tension on the h, value cannot be denied. Comparison of Present Data with Previous Correlations. Figures 11and 12 compare the present data with the previous correlations described above. In these figures, the Stanton numbers observed in the present work are plotted on logarithmic coordinates against the Stanton numbers calculated from the previous correlations. Figure 11 shows the comparison of the present data with the correlation proposed by Deckwer (1980). It can be seen that the data points fall some 10 to 50% above the solid line representing the Deckwer correlation and the largest difference between the observed and calculated Stanton numbers occurs at high values of the abscissa, corresponding to the low gas velocities. In Figure 12 the comparison of the present data with the correlation of Nishikawa et al. (1977) is shown. In calculating the values of the Stanton number, the (pw/p) term in eq 2 was assumed
Ind. Eng. Chem. Process Des. Dev., Vol. 20, No. 3, 1981 0.041
I
AV
Keys same as in Fig.9
0.002 0.002
4
I
6
I
I 1
6 0.01
1
2
I
0.03
(hw/PCpUdcal
Figure 11. Comparison of present data for Stanton number with Deckwer correlation. 0041
I
AV.
Keys same as in Fig. 9
v
0.002 0.002
4
6
I
,
8 0.01
2
1
0.03
(hw@cpuG )tal
Figure 12. Comparison of present data for Stanton number with correlation of Nishikawa et al.
to be unity. As can be seen from this figure, the correlation of Nishikawa et al. yields Stanton numbers about 25% lower than the present data. Conclusions To investigate the effect of the liquid physical properties on the heat transfer rate between the column wall and the aerated liquid in the bubble column with a single nozzle gas sparger, heat transfer experiments were carried out at relatively high gas velocities by using air and various li-
545
qui& of different physical properties. A new dimensionless correlation for the heat transfer coefficient was presented and shown to correlate well the experimental data with an average deviation of 3.9%. Nomenclature c = specific heat of liquid, J/kg K I& = nozzle diameter, m DT = column diameter, m g = gravitational constant, m/s2 h, = heat transfer coefficient, W/m2 K 12 = thermal conductivity of liquid, W/m K tL = liquid temperature, K or “C UG = superficial gas velocity, m/s uL = superficial liquid velocity, m/s 2, = aerated liquid height, m 2, = clear liquid height, m 2, = height of heat transfer section above bottom of column, m Ap = density difference between liquid and gas, kg/m3 EG = fractional gas holdup, dimensionless p = viscosity of liquid, Pa s p, = viscosity of liquid at wall temperature, Pa s p = density of liquid, kg/m3 u = surface tension of liquid, J/m2 Literature Cited Burkei, W. Chem. 1%. Tech. 1972, 44, 265. Deckwer, W. D. Chem. Eng. Sci. 1960. 35, 1341. Falr, J. R.; Lambright. A. J.; Andersen, J. K. Ind. Eng. Chem. Process Des. Dev. 1962, 1 , 33. Hart, W. F. Ind. Eng. Chem. ProcessDes. Dev. 1976, 15, 109. Hikita, H.; Asai, S.; Tanigawa, K.; Segawa, K.; Kltao, M. Chem. €ng. J. 1980, 20, 59. Hikita, H.; Asai, S.; Tanigawa, K.; Segawa, K.; Kltao, M. Chem. €ng. J. 1961, 22, 61. Huberiant, J. Sucr. Be& 1959, 78, 326. Kast, W. Int. J. Heat Mess Transfer 1962, 5. 329. Kast. W. Chem. Ing. Tech. 1969, 35, 705. KBlbei, H.; Siemes, W.; Maas, R.; Mirller, K. Chem. Ing. Tech. 1956, 30, 400. Koibei, H.; Borchers, E.; Martins, J. Chem. Ing. Tech. 1960, 32, 84. Konsetov, V. V. Int. J. Heat Mess Transfer 1966, 9 , 1103. McAdams, W. H. “Heat Transmission”, 3rd ed.; McQlaw-HiH: New York, 1954; p 404. Nishikawa, M.; Kato, H.; Hashimoto, K. Ind. Eng. Chem. Recess Des. Dev. 1977, 16, 133. Perry, J. H.; Chilton, C. H. “Chemical Engineers’ Handbook”, 5th ed.; McGraw-Hili: New York, 1973 pp 3-126, 3-136. Reid, R. C.; Prausnitz, J. M.; Sherwwd, T. K. “The Properties of Qases and LiquMs”, 3rd ed.; McGraw-HiiI: New York, 1977; p 522. Rfflick, J. A.; Bunger, W. B. “Organic Solvents”. 3rd ed.;Wiley-Interscience: New York, 1970; p 44. Riedei, L. Chem. Ing. Tech. 1949, 21, 340. Riedei, L. Chem. Ing. Tech. 1951, 23. 465. Ruckenstein, E.; Smigeischi, 0. Trans. Inst. Chem. Eng. 1965. 43, T334. Steiff. A.; Weinspach. P. M. Ger. Chem. Eng. 1978, 1 , 150. Yoshtome, H.; Mannami, Y.; Mukai, K.; Yoshlkoshi, N.; Kanazawa, T. K8@3ku Kogaku 1965, 29, 19.
Received for reuiew November 10,1980 Accepted April 13, 1981
