Kinetics and thermodynamics of the phosphine adsorption on the modified activated carbon

Abstract

The kinetics and the thermodynamics of phosphine (PH₃) adsorption on the modified activated carbon have been explained for the adsorption process of PH₃. This study investigated the kinetic and thermodynamic properties of PH₃ adsorption on the activated carbon impregnated with 5% HCl solution. The thermodynamic properties including PH₃ adsorption isotherm and adsorption heat were separately investigated at 20°C, 70°C, 90°C. The results showed that the Freundlich-type isotherm equation described the isotherms well. The adsorption capacity increased with increasing temperature between 20°C and 70°C. Between 70°C and 90°C, the adsorption capacity decreased obviously with increasing temperature. The adsorption capacity reached the maximum at 70°C. By analyzing the results of the kinetics and the thermodynamics, we found that the adsorption of PH₃ was dominated by physical adsorption at the lower temperature (20°C). Then with increasing temperature, chemical adsorption gradually dominated in the adsorption process. The adsorption capacity decreased at above 70°C is due to the exothermic effects in the process of adsorption.

Keywords

adsorption / PH₃ / activated carbon / kinetics / thermodynamics

References

[1] Chen S J. The current production status and consumption ways of phosphorus in China. Chemical Industry and Engineering Progress, 2005, 21: 776–778 (in Chinese)

[2] Ma L, Ning P, Zhang Y, Wang X. Experimental and modeling of fixed-bed reactor for yellow phosphorous tail gas purification over impregnated activated carbon. Chemical Engineering Journal, 2008, 137(3): 471–479

[3] Quinn R, Dahl T A, Toseland B A. An evaluation of synthesis gas contaminants as methanol synthesis catalyst poisons. Applied Catalysis A, 2004, 272: 61–68

[4] Sun H, Hankins N P, Azzopardi B J, Hilal N, Almeida C A P. A pilot-plant study of the adsorptive micellar flocculation process: Optimum design and operation. Separation and Purification Technology, 2008, 62(2): 273–280

[5] Wang X, Ning P, Shi Y, Jiang M. Adsorption of low concentration phosphine in yellow phosphorus off-gas by impregnated activated carbon. Journal of Hazardous Materials, 2009, 171(1–3): 588–593

[6] Quinn R, Dahl T A, Diamond B W, Toseland B A. Removal of arsine from synthesis gas using a copper on carbon adsorbent. Industrial & Engineering Chemistry Research, 2006, 45(18): 6272–6278

[7] Bandosz T J. Effect of pore structure and surface chemistry of virgin activated carbons on removal of hydrogen sulfide. Carbon, 1999, 37(3): 483–491

[8] Bandosz T J. On the adsorption/oxidation of hydrogen sulfide on activated carbons at ambient temperatures. Journal of Colloid and Interface Science, 2002, 246(1): 1–20

[9] Alhamed Y A. Adsorption kinetics and performance of packed bed adsorber for phenol removal using activated carbon from dates’ stones. Journal of Hazardous Materials, 2009, 170(2–3): 763–770

[10] Bagreev A, Rahman H, Bandosz T J. Study of H₂S adsorption and water regeneration of spent coconut-based activated carbon. Environmental Science & Technology, 2000, 34(21): 4587–4592

[11] Tsai J H, Jeng F T, Chiang H L. Removal of H₂S from exhaust gas by use of alkaline activated carbon. Adsorption, 2001, 7(4): 357–366

[12] Bagreev A, Rahman H, Bandosz T J. Wood-based activated carbons as adsorbents of hydrogen sulfide: a study of adsorption and water regeneration processes. Industrial & Engineering Chemistry Research, 2000, 39(10): 3849–3855

[13] Siriwardane R V, Shen M S, Fisher E P, Poston J A. Adsorption of CO₂ on molecular sieves and activated carbon. Energy & Fuels, 2001, 15(2): 279–284

[14] Adib F, Bagreev A, Bandosz T J. Analysis of the relationship between H₂S removal capacity and surface properties of unimpregnated activated carbons. Environmental Science & Technology, 2000, 34(4): 686–692

[15] Li W C, Bai H, Hsu J N, Li S N, Chen C. Metal loaded zeolite adsorbents for phosphine removal. Industrial & Engineering Chemistry Research, 2008, 47(5): 1501–1505

[16] Huang C C, Chen C H, Chu S M. Effect of moisture on H₂S adsorption by copper impregnated activated carbon. Journal of Hazardous Materials, 2006, 136(3): 866–873

[17] Xiao Y, Wang S, Wu D, Yuan Q. Catalytic oxidation of hydrogen sulfide over unmodified and impregnated activated carbon. Separation and Purification Technology, 2008, 59(3): 326–332

[18] Ren B N. Factors influencing adsorption of PH₃ on modified activated carbon. Advanced Materials Research, 2009, 79–82: 39–42

[19] Zhang K, Hong J, Cao G, Zhan D, Tao Y, Cong C. The kinetics of thermal dehydration of copper(II) acetate monohydrate in air. Thermochimica Acta, 2005, 437(1–2): 145–149

[20] Karlin K D, Kaderli S, Zuberbühler A D. Kinetics and thermodynamics of copper(I)/dioxygen interaction. Accounts of Chemical Research, 1997, 30(3): 139–147

[21] Zou W H, Han R P, Chen Z, Shi J,Liu. Characterization and properties of manganese oxide coated zeolite as adsorbent for removal of Copper (II) and Lead(II) ions from solution. Journal of Chemical & Engineering Data, 2006, 51(2): 534–541

[22] Li S F. Chemical Reaction Engineering. Beijing: Chemical Industry Press, 2005, 66–67 (in Chinese)

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