co2 k2o

2nd Conference on Chemical Engineering and Advanced Materials (CEAM)

VIRTUAL FORUM November 15th - 26th, 2010

Copyright 2010 Praise Worthy Prize S.r.l. - All rights reserved

Kinetics Study of Carbon Dioxide Absorption into Aqueous Potassium Carbonate Promoted with Boric Acid

L. Pudjiastuti1, E.A.Saputra2, A.Altway3, Susianto4, Kuswandi5

Abstract Many commercial processes for removal of carbon dioxide from acid gases have used aqueous potassium carbonate promoted with amines. This paper presents kinetic data and absorption rate for aqueous potassium carbonate promoted with boric acid. Kinetics of the absorption of CO2 into 30 wt% potassium carbonate promoted with boric acid were investigated at 30, 40, 50oC by using a wetted-wall column apparatus. The addition of 0.162 0.485 mol.l-1 boric acid to 30 wt% potassium carbonate system results in a significant enhancement of CO2 absorption rates. Based on pseudo-first order for CO2 absorption, pseudo-first order reaction rate constants were determined from the measured kinetics data. The reaction rate constants for boric

acid promoted absorption are [ ]7 7 2202 9 23 10 1 42 101 00 10 . . . . KBOk . . exp RT =

and

[ ]2

2 397202 2

1 27296 2325 10 .KBO.k . . exp KBORT

= with average deviation 12,11% and 1,35%

respectively. Copyright 2010 Praise Worthy Prize S.r.l. - All rights reserved. Keywords: Absorption, CO2 Removal, Kinetics, Promoter, Boric Acid

Nomenclature d DCO2 g h k1 k1boric cid k1 k2 k2,boric acid k2,boric acid kg Q q r R Re Sc Sh t

Diameter of Wetted Wall Column, m Diffusivity of dissolved CO2, m2/s Gravitational acceleration, m/s2 Height of Wetted Wall Coulumn, m Rate constant of overall reaction, 1/s Rate constant of overall reaction with

boric acid, 1/s Second-order rate constant of reaction,

m3 / kmol.s Second-order rate constant of reaction

with promotor, m3 / kmol.s Second-order rate constant of reaction

with boric acid, m3 / kmol.s k2,boric acid x [ KBO2] ,1/s. Gas phase mass transfer coeficient, kmol/ m2 .s Quantity of gas absorbed by unit area in

time of contact t, kmol/m2

absorption rate (kmol/s) Rate of reaction, kmol/(m3.s) Gas constant, m3.Pa/kmol.K Reynold Number. Schmidt Number. Sherwood Number. contact time, s

T u us v V

Temperature, (K) Distribution of velocity in film, m/s Velocity in film surface , m/s. Liquid flow rate, m3/s. Volume of liquid, m3 Thickness of liquid film, m Viscosity of liquid, kg /m.s Density of liquid, kg/m3

I. Introduction Removal of acid gases, e.g. carbon dioxide (CO2), by

using reactive absorption with aqueous alkonalamine or potassium carbonate solution is an important industrial operation. The advantage of using alkanolamine solvent is its high reaction rate with carbon dioxide. Several investigators have explored the reaction rate of carbon dioxide is un-promoted, promoted and blended aqueous amines solution ([1] [7]). A problem with the use of alkanolamines for carbon dioxide removal is that they degrade as a result of long exposure or repeated use. Several attempts have been made to use alternative more stable solvent having high enough reaction rate with carbon dioxide for example amino acid salts [8]. The absorption of CO2 with potassium carbonate solvent has gained widespread and has been accepted for removal of CO2 from the natural and synthetic gas stream due to its stability, low cost and low energy requirement for

L. Pudjiastuti, E.A.Saputra, A.Altway, Susianto, Kuswandi

Copyright 2010 Praise Worthy Prize S.r.l. - All rights reserved 2nd Conference on Chemical Engineering and Advanced Materials (CEAM)

solvent regeneration. However, the reaction rate between carbon dioxide with potassium carbonate is lower than the reaction rate with amines solution ([9], [10])

Several researchers have shown that the application of piperazine/amines-promoted potassium carbonate could accelerate the absorption process ([11] [15]). However, many promoters are carcinogenic in nature and some others are not stable at stripper conditions. In this case, boric acid is environmental friendly.

There is some information available regarding the absorption of carbon dioxide using aqueous solution of potassium carbonate promoted with boric acid [16]. But none of the literature discussed the detailed kinetics of the reaction of carbon dioxide in the liquid phase for boric acid promoted potassium carbonate solvent system. The detailed kinetics of the reaction is essential for the process design and simulation of CO2 absorption in boric acid promoted potassium carbonate solvent.

This work focuses on expanding the investigation of promoted potassium carbonate (K2CO3) by using boric acid. The main purpose of this work is to investigate the effect of boric acid on the reaction rate constant of CO2 absorption into aqueous potassium carbonate solution by using a laboratory wetted wall column. Experimental kinetic data were collected. A simplified model used to interpret the results.

II. Theory II.1. Reaction system

The absorption of CO2 into aqueous K2CO3 is commonly represented by overall reaction

( )3 2 2 32CO H O CO aq HCO + + (1)

The reaction is usually described in term of two parallel, reversible reactions. ( )2 3CO aq OH HCO + (2)

23 3 2HCO OH CO H O

+ + (3)

Since the reaction with hydroxide is the rate-limiting step, the forward reaction rate is represented as a second order rate expression.

[ ]

2 2CO OHr k OH CO = (4)

This reaction, though important to the solution

equilibrium, is generally much slower than aqueous amines, limiting its application in processes requiring a high percentage of removal. It is often advantageous to add a promoter to increase the absorption rate. The energy required to reverse the reaction is typically less than that required for amine solvents.

The rate equation for the reaction of carbon dioxide with unpromoted hot potassium carbonate is ([3], [12])

[ ] [ ]( )2 2OH OH er k OH CO CO = (5)

The carbonate-bicarbonate system is buffer solution; hence the concentration of OH- ion in the solution near the surface of the liquid is not significantly affected by the absorption of CO2. In this case, carbon dioxide undergoes a pseudo-first-order reaction and Eq. (4a) can be rewritten as ([3], [13])

[ ] [ ]( )1 2 2OH er k CO CO= (6)

When H3BO3 is added to the carbonate-bicarbonate solution, the absorption process occurs via several mechanisms. A convenient procedure for adding potassium borate to the potassium carbonate scrubbing solution is by adding boric acid, whereupon the boric acid is converted to potassium borate in accordance with the following reaction [10]: 3 3 2 3 2 2 22 2 3H BO K CO KBO CO H O+ + + (7)

In this event, the potassium carbonate content of the solution must be properly adjusted to compensate for that consumed by reaction with the added boric acid.

The main role played by buffer solution, when KBO2 is present, is that of creating a medium in which the salt can dissociate and then the catalytic activity may be exploited. The rate equation for the catalyzed reaction, which is always first-order with respect to carbon dioxide, can be written in the following way [2]:

[ ]2promoter promoterr k CO= (8)

2 2promoter KBOr k BO = (9)

Using the same approach for deriving Eq (5), gives

the following pseudo-first-order rate equation of carbon dioxide with activated potassium in liquid phase:

[ ]( ) [ ] [ ]( )2 2 2 2KBO er k KBO CO CO= (10)

Eqs.(5) and (10) lead to overall pseudo-first-order rate equation of carbon dioxide with activated potassium carbonate in liquid phase:

[ ]( ) [ ] [ ]( )2 2 2 2 2KBO KBO er

k OH k KBO CO CO=

+ (11)

[ ] [ ]( )1 2 2 er k ' CO CO= (12)



where k is the overall apparent first-order rate constant and is defined as [12], ( )21 2OH KBOk ' k OH k BO = + (13)

The rate constant has been measured by [3]

289513 635 0 08OHlog k , , IT = (14)

II.2. Wetted Wall Column

Wetted Wall column is equipment commonly used to study the kinetics of gas-liquid reaction. The liquid flow in the wetted wall column is usually maintained in laminar pattern. In this case the gas-liquid contact time is determined as follows,

s

htu

= (15)

where su is the liquid surface velocity given by

2

2sgu = (16)

and is the film thickness given by

3 3 solQgW

= (17)

If Q( t ) is amount of gas absorbed by unit area of surface during a contact-time t, the total rate of absorption q into the film is related to Q( t ) by

Q(t) q

dht= (18)

The absorption rate q is usually measured experimentally. Then, equation (19) can be used to determine the value of pseudo first-order reaction rate constant of reversible reaction using the experimental absorption rate data:

( )Ai Ae 1Q C C At D k= (19)

where:

1

1

G A A AeAi

G A

k P D k CC

k He D k+= + (20)

- 22 3

2-1 2

K [HCO ]K [CO ]Ae

C = (21)

II.3. Gas film mass transfer coefficient

The gas film mass transfer coefficient, kg, in the wetted-wall column was determined as in [13] using SO2 absorption into 0.1 M NaOH. The results of the experiments are correlated as in equation (22)

0 85

1 075,dsh , Re Sc

h = (22)

The Reynolds number is defined as:

u dRe = (23)

The Schmid number is:

2Sc

DCO

= (24)

The gas film transfer coefficient can be found from

the following definition of the Sherwood number

2g COSh RTk h / D= (25)

III. Experimental Procedure The wetted-wall column, depicted in Fig.1 and 2, was

used as the gas-liquid contactor throughout the kinetic data and absorption rate measurement. The contactor is the same equipment as used in the work of [5],[8], and [14]. The stainless steel, 9.3-cm in height and 1.3 cm in outside diameter, is a tube extending from the liquid feed line into the column. The liquid is pumped through the inside of the tube, overflows, and is evenly distributed across the outer surface of the tube. Gas enters near the base of the column, counter-currently contacting the fluid as it flows up to the gas outlet. The liquid flow rate was varied in the range 5-10 cm3/s. The gas flow rate is 100 cm3/s . The CO2 absorption rate was measured from the difference in inlet and outlet CO2 composition in the gas as determined using by Orsat apparatus.

IV. Results and Discussion IV.1. Absorption Rates

The absorption experiments for CO2 into potassium carbonate solution (30 mass % K2CO3) with the addition of boric acid were carried out over the concentration range 0.162 0.485 mol.l-1. The experiments were carried out over the temperature range of 303 to 323 K. All experiments were performed under atmospheric pressure with partial pressure of CO2 near atmospheric pressure.



C : Heater P1 : Promoted K2CO3

pump. P2 : Water pump. R1 : Liquid rotameter. R2 : Gas rotameter. T1 : Waterbath T2 : Promoted K2CO3

tank. T3 : Overflow tank. T4 : CO2 tank T5 : Sample tank. t :Thermocouple V1 : Liquid Valve V2 : CO2Valve V3 WWC

:Valve ( by pass ) :Wetted wall column.

Fig. 1. Experimental Apparatus

Fig. 2. Wetted Wall Column

Table I are the rate of CO2 absorption as measured in

the wetted wall column, where solution 1(Sol-1) is the addition of boric acid 1wt% into 30wt% K2CO3; solution 2(Sol-2) is the addition of boric acid 2 wt% into 30wt% K2CO3 and solution 3(Sol-3) is the addition of boric acid 3 wt% into 30wt% K2CO3.

The CO2 absorption rate in various solutions is plotted in Fig 3, 4, and 5. Increasing the boric acid concentration from 1wt% to 3 wt% affects the CO2 absorption rate enhancement by a factor of 1.63. CO2 absorption rate increase by factor of 3.99 with increasing volumetric rate from 5 m3/s to 10 m3/s .

The effect of temperature on rate of CO2 absorption is shown in figures 6, 7 and 8. It can be seen from that figures, that the average CO2 absorption rate increase by factor of 1.384 as temperature increases from 303K to 323K .

TABLE I EXPERIMENTAL RESULT OF ABSORPTION RATE

v x 106 t T q x 108

kmol/s m3/s s K Sol-1 Sol-2 Sol-3

5 0.817

303

2.001 3.982 5.211 6.667 0.675 4.965 5.944 7.548 8.333 0.581 5.944 10.765 12.188 10 0.515 9.810 14.537 16.536

5

0.817

313

2.994

4.965

5.944

6.667 0.675 5.944 6.918 7.886 8.333 0.581 8.850 11.715 12.660

10 0.515 11.715 14.537 16.536 5

0.817

323

3.982

4.965

6.918

6.667 0.675 7.886 9.810 9.810 8.333 0.581 10.765 12.660 13.601

10 0.515 12.660 15.469 17.320

Fig. 3. CO2 absorption rate in various solutions at temperature 303K

Fig. 4. CO2 absorption rate in various solution at temperature 313K

Fig. 5. CO2 absorption rate in various solutions at temperature 323K



Fig. 6. CO2 absorption rate in Sol-1 in various temperature

Fig. 7. CO2 absorption rate in Sol-2 in various temperature

Fig. 8. CO2 absorption rate in sol-3 in various temperatures

IV.2. Kinetics of CO2 Reaction with Potassium Carbonate and Boric Acid

CO2 react with aqueous solution of potassium carbonate as follow:

2 3CO OH HCO

+ (26) 3 3CO H HCO

= + + (27)

2 2 3CO H O H HCO+ + + (28)

3 2 3CO H O HCO OH= + + (29)

Both reactions (26) and (28) are slow and rate

determining [13]. Reaction rate constant (k1) for the equation (26) is shown in Table II.

TABLE II

REACTION RATE CONSTANT OF EQUATION (26) Temperature, K k1(m3/kmol.s) Reff 303 12170

[9] 313 24560 323 36950

Reaction rate constant for CO2 absorption into boric

acid promoted K2CO3 solution was determined experimentally in this work, and is shown in Table III and IV.

TABLE III

EXPERIMENT RESULT OF REACTION RATE CONSTANT IN EQUATION (28)

Solution k2. 10-4 ( m3/kmol.s )

303 K 313 K 323 K

Sol-1 3.006 10.851 33.708

Sol-2 9.212 20.933 63.026

Sol-3 18.658 40.081 161.599 Table III shows the reaction rate constant for

equation (28) as measured in the wetted wall column.

TABLE IV EXPERIMENTAL RESULT OF REACTION RATE CONSTANT

Solution k1' . 10-4 ( 1/s ) k2' . 10-4 ( 1/s )

303 K 313 K 323 K 303 K 313 K 323 K

Sol-1 0.488 1.761 5.464 0.486 1.755 5.452

Sol-2 2.981 6.775 20.397 2.980 6.771 20.387

Sol-3 9.054 19.451 78.416 9.053 19.447 78.408

Reaction rate constant (k2) is affected by temperature and concentration of boric acid. Addition of boric acid with concentration in the range 1wt% to 3 wt% into 30% potassium carbonate solution and temperature range from 303 K to 323 K, increases reaction rate constant significantly.

The reaction rate constant (k2) for various solution are plotted in Fig. 9 and are fitted by the following equation (model-1)

[ ]7 7 220

29 23 10 1 42 10

1 00 10( . . . . KBO

k . . expRT

= (30)

Equation (30) indicates that addition of boric acid in

range 1-3 wt%, decreases the activation energy, and so increases k2.



Average Relative Deviation (ARD) of k2 from equation (30) and experimental data is shown in Table V.

Fig. 9. Reaction rate constant in various temperature

From Table V, average deviation (ARD) of the second-order rate constant of reaction with promotor is lower than 15%. This reaction rate model is found to be satisfactory in representing the CO2 absorption into K2CO3+ KBO3 + H2O systems

The reaction rate constant (k2KBO2) for various solution are plotted in Fig.10 and are fitted by the following Arrhenius equation (model-2):

[ ]2

2 397202 2

1 27296 2325 10 .KBO.k ' . . exp KBORT

= (31)

TABLE V AVERAGE DEVIATION OF EQUATION (30)

T [KBO2] k2 * 10-5

eksperiment k2 (Eq 30 ) deviation

( K ) (kmol/m3) (m3/kmol.s) (m3/kmol.s)

303 0.16173 0.3007 3.077.E+04 2%

313 0.16173 1.085 9.631.E+04 11%

323 0.16173 3.371 2.809.E+05 17%

303 0.32347 92.12 7.646.E+04 17%

313 0.32347 2.093 2.325.E+05 11%

323 0.32347 6.303 6.599.E+05 5%

303 0.48520 1.866 1.900.E+05 2%

313 0.48520 4.008 5.612.E+05 40%

323 0.48520 161.6 1.550.E+06 4%

ARD = 12.11%

Average Relative Deviation (ARD) of k2 from

equation (31) and experiment is shown in Table VI. From Table VI, average deviation (ARD) of the

pseudo first-order rate constant of reaction with promotor is 1.35%. This reaction rate model is found to be satisfactory in representing the CO2 absorption into

K2CO3+ KBO3 + H2O systems. This kinetic model is better than the first model.

Fig. 10. Reaction rate constant in various temperature

Fig. 11. Comparison of overall reaction rate constant (k1boric acid). The kinetic model in Eqs.(31) were compared with

the available literature data: for MDEA blended with DEA [3]; K2CO3+ PZ [13]; MEA [3]; PZ and MDEA [5]. Fig. 11 show the comparison of the overall reaction rate constant ( k1KBO2) from this work with the available literature values.

As shown in Fig. 11, the calculated value of k1KBO2 from this work appear to be comparable with most available literature data.



TABLE VI AVERAGE DEVIATION OF EQUATION (31)

T [KBO2] k2 experiment k2 (eq. 31) deviation

( K ) (kmol/m3) (1/.s) (1/s)

303 0.16173 30065.0643 30766.2532 0.26%

313 0.16173 108520.3163 96308.2032 1.25%

323 0.16173 337103.1421 280908.8011 1.85%

303 0.32347 92121.5208 76461.5334 1.89%

313 0.32347 209325.5231 232487.7614 1.23%

323 0.32347 630265.2363 659861.4003 0.52%

303 0.48520 186575.5100 190025.2866 0.21%

313 0.48520 400807.0510 561224.8736 4.45%

323 0.48520 1615986.9518 1550029.9950 0.45%

1.35%

V. Conclusion Kinetics of the absorption of CO2 into potassium

carbonate solution (30 wt % K2CO3) with the addition of boric acid was investigated at 303,313, and 323 K using a laboratory wetted wall column. Three system of which 30 wt % K2CO3 with 1,2 and 3 wt% boric acid were studied. The addition of 1,2, and 3 wt% boric acid to 30 wt% potassium carbonate system results in a significant enhancement of CO2 absorption rates. Two kinetic models were proposed in this work. The first model, based on second-order reaction rate constant measurement, give the average deviation (ARD) of 12.11%. While the second model, based on pseudo first-order reaction rate constant measurement, gives the average deviation (ARD) of 1.35%. The latter kinetic model is found to be more satisfactory in representing the CO2 absorption into K2CO3+ KBO3 + H2O systems.

Acknowledgements The authors wish to acknowledge the financial

support of: - Guru Besar research grant administered by the

Department of Research and Social Services, Institute Technology of Sepuluh Nopember, Surabaya , Indonesia.

- Research Grant Program for Doctoral Students by Directorate of Higher Education, The Ministry of National Education of Indonesia.

References [1] J.Xiao, C.Li, Li, Kinetics of absorption of carbon dioxide into

aqueous solution of 2-amino-2-methyl-1-propanol + monoethanolamine. Chemical Engineering Science 55(1998) 161-175.

[2] H. Dang, G.T. Rochelle, CO2 absorption rate and solubility in Monoethanolamine/Piperazine/Water, The First National Conference on Carbon Sequestration, Washington, DC, Mei 14-17 (2001).

[3] Z.Xu, Y.Yanhua, Z.Chengfang, Absorption rate of CO2 into MDEA Aqueous solution blended with piperazine and diethanolamine. Chinese Journal Chem. Eng. 11(4) (2003) 408-413.

[4] S.Paul,A.K.Ghoshal, B.Mandal , Kinetics of absorption of carbon dioxide into aqueous solution of 2-(1-piperazinyl)-ethylamine, Chemical Engineering Science 64 (2009) 313-321

[5] S. Paul, A.K. Ghosal, B.Mandal, Kinetics of absorption of carbn dioxide into aqueous blends of piperazine and methyldiethanolamine. Chemical Engineering Science 64 (2009) 1618-1622.

[6] A.Hartono, E.F. da Silva, H.F.Svendsen,Kinetics of carbon dioxide absorption in aqueous solution of diethylenetriamine (DETA), Chemical Engineering Science 64 (2009) 3205-3213

[7] R.Idem, M.Edali, A.Aboudheir, Kinetics, Modeling, and Simulation of the Experimental Kinetics Data of Carbon Dioxide Absorption into Mixed Aqueous Solutions of MDEA and PZ using Laminar Jet Apparatus with a Numerically Solved Absorption-Rate/Kinetic Model,Energy Procedia 1 (2009) 1343-1350

[8] J. Van Holst, G.F. Versteeg, D.W.F. Brilman, J.A. Hogendoorn, Kinetic study of CO2 with various amino acid salts in aqueous solution, Chemical Engineering Science 64 (2009) 59-68

[9] Benson, J.H.Field, W.P. Haynes, Improved process for CO2 absorption uses hot carbonate solutions, Chemical Engineering Progress 52 (1956) 433-438

[10] G. Astarita, D.W. Savage, and A. Bisio, Gas treating with Chemical Solvent (Wiley, 1983), New York.

[11] H. Bosch, G.F. Versteeg, W.P. Van Swaaij, Gas-liquid mass transfer with parallel reversible reactins-II. Absorption of CO2 into amine-promoted carbonated solution. Chemical Engineering Science 44(11) (1989) 2735-2743.

[12] V.Augugliaro, L.Rizzuti, Kinetics of carbon dioxide absorption into catalysed potassium carbonate solutions, Chemical Engineering Science 42 (1987) 2339-2343.

[13] J.T. Cullinane, G.T. Rochelle, Carbon Dioxide Absorption with Aqueous Potassium Carbonate Promoted by Piperazine, Chemical Engineering Science 59 (2004) 3619-3630.

[14] M.R. Rahimpour, A.Z. Kashkool, Modeling and Simulation of Industrial Carbon Dioxide Absorber Using Amine-Promoted Potash Solution, Iranian Journal Of Science & Technology, Transaction b 28 B6 (2004)

[15] M.R. Rahimpour, A.Z. Kashkool, Enhanced Carbon Dioxide Removal by Promoted Hot Potassium Carbonate in a Split-Flow Absorber, Chemical Enginering and processing 43 (2004) 857-865.

[16] U.K. Gosh, S.E. Ketish, G.W. Stevens, Absorption of carbon dioxide into aqueous pottasium carbonate promoted by boric acid. Energy Procedia 1( 2009) 1075-1081.

Authors Information First Authors name: Lily Pudjiastuti Place and date of birth: Banjarmasin, Indonesia, July 03th 1958. Educational background: Bachelor s degree in Chemical Engineering from Institut Teknologi Sepuluh Nopember (ITS) Surabaya, Indonesia in 1983; Masters degree in Chemical Engineering from Institut Teknologi Sepuluh Nopember

(ITS) Surabaya, Indonesia in 2002.

Second Authors name: Erwan Adi Saputra, Place and date of birth: Surabaya, Indonesia, August 03th 1980. Educational background: Bachelors degree in Chemical Engineering, from Institut Teknologi Sepuluh Nopember,Surabaya, Indonesia in 2002.



Third Authors name: Ali Altway Place and date of birth: Jakarta, Indonesia. August 4, 1951 Educational background: Masters degree in Chemical Engineering from the University of Wisconsin , Madison, WI, USA in 1979; Doctorate in Chemical Engineering from Sepuluh Nopember Institute of

Technology, Surabaya, Indonesia in 2004. Dr. Altways major field of study is transport phenomena. Dr. Altway has authored several articles: 1. "Effect of Particle size on simulation of three-dimensional solid dispersion in stirred tank", TransIchemE., Vol. 79, No. A8, pp. 1011-1016 (2001); 2. Mass Transfer and Chemical Reaction Aspects Concerning Acetaldehyde Oxidation in Agitated Reactor, Studies in Surface Science and Catalysis, Vol. 159 (2006); 3. Numerical Analysis of Macro-Instability Characteristic in a Stirred Tank by Means of Large Eddy Simulations: Off-Bottom Clearance Effect ,Chemical Product and Process Modeling, Vol.3, Iss.1, Article 45 (2008); and 4. Effects of Feed Rate and Residence Time on Environment of Rotary Dryer Processes in Applied Science in Environment Sanitation, vol.4, No.1, January-April 2009.

Fourth Authors name: Susianto Place and date of birth: Tegal, Indonesia. August 20, 1962 Educational background: Masters degree in Chemical Engineering from the Institut National Polytechnique de Lorraine (INPL), Nancy, France in 1996. Doctorate in Chemical Enginnering from the Institut National

Polytechnique de Lorraine (INPL), Nancy,France in 2001. Dr. Susiantos major field of study is reaction engineering. Dr. Susianto has authored one article: Effects of Feed Rate and Residence Time on Environment of Rotary Dryer Processes in Applied Science in Environment Sanitation, vol.4, No.1, January-April 2009.

Fifth Authors name: Kuswandi Place and date of birth: Sumenep, Indonesia, June 12, 1958. Educational background: Masters degree in Chemical Engineering from the Universite de Technologie de Compiegne (UTC), Compiegne, France in 1996. Doctorate in Chemical Engineering from the Universite de

Technologie de Compiegne (UTC), Compiegne, France in 2000. Dr. Kuswandis major field of study is thermodynamics. Dr. Kuswandi has authored several articles: 1. "Dtermination Exprimentale des Equilibres Liquide-Vapeur de Binaires Htro-azotropiques", Entropie, No. 215, 1998; 2. "Separation of Hydrocarbon by Liquid Surfactant Membranes, Rcent Progrs en Gnie des Procds, No.68, Vol.13, 1999; and 3. "Effects of Feed Rate and Residence Time on Environment of Rotary Dryer Processes" Applied Science in Environment Sanitation, vol.4, No.1, January-April 2009.

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