Kinetics of Ferrous Sulfate Catalytic Oxidation from Dissolved Iron Waste in Sulfuric Acid

  • Hary Sulistyo Department of Chemical Engineering, Faculty of Engineering, Gadjah Mada University, 55281 Yogyakarta, Indonesia
  • Suprihastuti Sri Rahayu Department of Chemical Engineering, Faculty of Engineering, Gadjah Mada University, 55281 Yogyakarta, Indonesia
  • Wahyudi B Sediawan Department of Chemical Engineering, Faculty of Engineering, Gadjah Mada University, 55281 Yogyakarta, Indonesia
  • Sarto Sarto Department of Chemical Engineering, Faculty of Engineering, Gadjah Mada University, 55281 Yogyakarta, Indonesia
  • Takdir Syarif Department of Chemical Engineering, Faculty of Industrial Technology, Indonesian Moslem University, Makassar, Indonesia

Abstract

Iron waste was dissolved in a sulfuric acid to form a concentrated FeSO4- H2SO4 solution This research was conducted by catalytic oxidation of ferrous sulfate using manganese dioxide as catalyst to form a ferric sulfate. Catalytic oxidation reaction using a catalyst of manganese dioxide is a three phase heterogeneous reaction. This reaction kinetics is quite complex. This study aims to develop a mathematical modeling of reaction kinetics for three phases, gas, liquid and solid. Oxidation was undertaken on the condition of isothermal and isobaric in the threeneck flask as reactor. Experiment was run in the temperature range of 313 K to 363 K and catalyst concentration of 4.16 10 -3 gL-1 to 25 10 -3 gL-1.

Results indicated that the oxidation rate increased with the increase of temperature and catalyst concentration. Reaction kinetics can be approached with quasi steady state model and chemical reactions on the surface of the catalyst are a step controls the reaction kinetics. The relation between reaction rate constant and temperature in the following Arrhenius form:

kR = 2182exp (-17613/RT),L g.eq-1min-1

Manganese dioxide as catalyst can increase a reaction rate and reduce the activated energy which can be expressed in the following equation

E = 20129.025exp(-0.0472mk),Jmol-1

Activated energy was found from 14414 Jmol-1to 19747 Jmol-1 and maximum ferrous sulfate conversion was of 97.20%. Those values were similar result with the literature available.

References

1. Cher, M., and Davidson, N. (1955). The Kinetics of the Oxygenation of Ferrous Iron in Phosphoric Acid Solution, Journal of Am. Chem. Soc., 77, 793-798.
2. Chmielewski, T., and Charewic, W.A. (1984). The Oxidation of Fe(II) in Aqueous Sulphuric Acid Under Oxygen Pressure, Hydrometallurgy, 12, 21- 30.
3. Fogler, H.S. (2006). Elements of Chemical Reaction Engineering, 4th, Prentice Hall International, Upper Saddle River, New Jersey.
4. Jenson, V.G., and Jeffreys, G.V. (1977). Mathematical Methods in Chemical Engineering, 2nd ed, Academic Press Inc., New York.
5. King, J., and Davidson, N. (1958). Kinetics of the Ferrous Iron-Oxygen Reaction in Acidic Phosphate- Pyrophosphate Solutions, Journal of Am. Chem. Soc., 80, 1542-1545.
6. Megawati, (2004). Kinetika Reaksi Oksidasi Fero Sulfat menjadi Feri Sulfat, Tesis Program Pasca Sarjana Univerasitas Gadjah Mada, Yogyakarta.
7. Perry, R. H., Green, D.W. and Maloney, J.D. (1984). Chemical Engineers Handbook, 6th ed, pp 3- 103, McGraw Hill International Book Company, Inc., New York.
8. Ronnholm, M.R., Warna, J., Salmi, T., Turunen, I. and Luoma, M. (1999a). Kinetics of Oxidation of Ferrous Sulfate with Molecular Oxygen, Chem. Eng. Sci., 54, 4223-4232.
9. Ronnholm, M.R., Warna, J., Salmi, T., Turunen, I. and Luoma. M. (1999b). Oxidation Kinetics of Ferrous Sulfate over Active Carbon, Ind. Eng. Chem. Res., 38, 2607-2614.
10. Sediawan, W.B., and Prasetya A., 1997., Pemodelan Matematis dan Penyelesaian Numeris dalam Teknik Kimia, ANDI, Yogyakarta.
11. Smith, J.M. (1981). Chemical Engineering Kinetics, 3rded, Mc Graw Hill Book Co, New York.
12. Sulistyo, H. (2003). Pengolahan Limbah Besi dengan Asam Sulfat Menjadi Feri Sulfat, Laporan Penelitian, Penelitian Dasar. DP4M Direktorat Pendidikan Tinggi.
13. Sulistyo, H., Wahyudi, R, and Astuti, D. (2003). Catalyzed Oxidation of Dissolved Iron Waste Ion to Ferric Sulfate, Proceeding Regional Symposium on Chemical Engineering (RSCE2003), Module B9, Manila December 1- 3. 2003
14. Sulistyo, H., and Yuwono, A. (2003). Heterogeneous Catalytic Oxidation of Dissolved Iron Waste over Manganese Oxide, Proceeding Regional Symposium on Chemical Engineering (RSCE2003). Module B9. Manila December 1- 3. 2003
15. Vogel. A.I. (1951). A Text Book of Quantitative Inorganic Analysis, 2nded. pp 268-276. Longmans. Green and Co. London.
Published
2009-12-31
How to Cite
Sulistyo, H., Rahayu, S. S., Sediawan, W. B., Sarto, S., & Syarif, T. (2009). Kinetics of Ferrous Sulfate Catalytic Oxidation from Dissolved Iron Waste in Sulfuric Acid. ASEAN Journal of Chemical Engineering, 9(2), 49-56. Retrieved from https://jurnal.ugm.ac.id/v3/AJChE/article/view/8058
Issue
Vol 9 No 2 (2009)
Section
Articles

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