Silvernano Particle Loaded on Activated Carbon as Novel Adsorbent for the Removal of Acid Yellow 199 Dye

الموضوعات :

Z. Alishavandi ¹ , N. Mosallanejad ² , R. shabani ³

1 - Graduate student, Department of Chemistry, Firozabad Branch, Islamic Azad University, Firozabad, Iran
2 - Department of Chemistry, Mashhad Branch, PN University, Khorasan, Iran
3 - Department of Chemistry, Firozabad Branch, Islamic Azad University, Firozabad, Iran

تاريخ الإرسال : 04 السبت , صفر, 1435 تاريخ التأكيد : 20 الإثنين , صفر, 1440 تاريخ الإصدار : 25 الأحد , شوال, 1434

الکلمات المفتاحية: Adsorption, kinetic, Acid Yellow 199, Silver nanoparticle loaded on activated carbon, equilibrium and thermodynamic,

ملخص المقالة :

In this study, a new adsorbent, silver nanoparticle loaded on activated carbon (Ag˗NP˗AC) was usedfor removal of acid yellow199 (AY 199) dye. This novel material was characterized and identified by differenttechniques such as Brunauer, Emmett and Teller (BET), field emission scanning electron microscopy(FESEM), X-ray diffraction (XRD) analysis. Unique properties of this adsorbent such as high surface area(>1100 m2g-1) and low pore size (<47 A˚) and average particle size lower than 60 A˚ make it possible forefficient removal of Ay199. In batch experimental set-up, adsorbent dosage, initial dye concentration, contacttime and pH were investigated. Optimum values were set as pH of 3.0, 0.03g/50mL of adsorbent for initial dyeconcentration of 15 mgL-1 at 40 min and 25 ±1 ºC. The adsorption of Ay199 follows the pseudo-second-orderrate equation in addition to interparticle diffusion model (with removal more than 90%) at all conditions.Equilibrium data fitted well with the Langmuir model, while maximum adsorption capacity was 30 mg g-1 for0.03 g/50mL of Ag˗NP˗AC. Calculation of various thermodynamic parameters such as, Gibb’s free energy,entropy and enthalpy of the on-going adsorption process also indicated feasibility and endothermic nature ofAY 199 adsorption onto Ag˗NP˗AC.

المصادر:

1. Heydari M., Fazaeli R., Yousefi M., 2012.
2. Preparation of PerovskiteNanocomposites
3. andPhotochemical Degradation Kinetics of Acid
4. Yellow 199, J.Appl.ChemRes, 6:7-15.
5. Wijetunga S., Xiufen L., Wenquan R., Chen J.,
6. Removal Mechanisms of Acid Dyes of
7. DifferentChemical Groups under Anaerobic
8. Mixed Culture, Ruhana J. Scie, 2: 96-110.
9. Blackburn R. S., 2004. Natural polysaccharides
10. and their interactions with dye molecules:
11. applications in effluent treatment. Environ. Sci.
12. Technol. 38: 4905ââ‚‌“ 4909.
13. Crini G.,Peindy H. N.,Gimbert F., 2007.
14. Removal of C.I. Basic Green 4 (Malachite Green)
15. from aqueous solutions by adsorption using
16. cyclodextrin- based adsorbent: Kinetic and
17. equilibrium studies. Sep. Pur. Technol, 53: 97ââ‚‌“
19. Sun Q., Yang L., 2003.The adsorption of basic
20. dyes from aqueous solution on modeled peatresinparticle.
21. Water Res. 37:1535-1544.
22. Yee H., Chin S. M., 2005. Decolorization
23. effects of six azo dyes by O3, UV/O3 and
24. UV/H2O2processes. Dyes Pigm. 65: 25-31.
25. Chatterjee S., Chatterjee S.,Chatterjee B. P.,
26. Guha A. K., 2007. Adsorptive removal of congo
27. red, a carcinogenic textile dye by chitosan
28. hydrobeads: Binding mechanism, equilibrium and
29. kinetics. Colloids & Surfaces A: Physicochem.
30. Eng. Aspects. 299:146ââ‚‌“152.
31. Mondal S., 2008. Methods of dye removal from
32. dye house effluent-an overview. Environ. Engg.
33. Sci. 25:383ââ‚‌“396.
34. Zonoozi M. H., MoghaddamM. R. A., Arami
35. M., 2009. Coagulation/flocculation of dye
36. containing solutions using polyaluminium chloride
37. and alum. Water Sci. Technol. 59:1343ââ‚‌“1351.
38. Sachdeva S., Kumar A., 2009. Preparation of
39. nanoporous composite carbon membrane for
40. separation of Rhodamine B dye. J. Membr. Sci.
41. : 2ââ‚‌“10.
42. Tan I., Ahmad A. L., Hameed B. H., 2008.
43. Adsorption of basic dye on high-surface area
44. activated carbon prepared from coconut husk:
45. equilibrium, kinetic and thermodynamic studies. J.
46. Hazard. Mater. 154:337ââ‚‌“346.
47. Gupta V. K., Jain R., Varshney S., 2007.
48. Electrochemical removal of hazardous dye
49. Reactofix Red 3 BFN from industrial effluents. J.
50. Colloid Interface Sci. 312: 292ââ‚‌“296.
51. Gupta V. K., 2007. Photochemical degradation
52. of hazardous dyeââ‚‌”safaranin-T using TiO2
53. catalyst. J. Colloid Interface Sci. 309: 460ââ‚‌“465.
54. Kavitha D., Namasivayam C., 2007.
55. Experimental and kinetic studies on methylene
56. blue adsorption by coir pith carbon. Bioresour.
57. Technol. 98:14ââ‚‌“21.
58. Hua Z., Chena H., Ji F., Yuana S., 2010.
59. Removal of Congo Red from aqueous solution by
60. cattail root. J. Hazard Mater. 173:292ââ‚‌“297.
61. Cheung W. H., Szeto Y. S., McKay G., 2009.
62. Enhancing the adsorption capacities of acid dyes
63. by chitosan nano particles.Bioresour. Technol.
64. :1143ââ‚‌“1148.
65. Mosallanejad N., Arami A., 2012. Kinetics and
66. isotherm of sunset yellow dye adsorption on
67. cadmium sulfide nanoparticle loaded on activated
68. carbon, J Chem Health Risks 2(1): 31-40.
69. Huang H., Yang X., 2004. Synthesis of
70. polysaccharide-stabilized gold and silver
71. nanoparticles: A green method. Carbohyd. Res.
72. , 2627-2631
73. Huang H., Yang X., 2004. Synthesis of
74. polysaccharide-stabilized gold and silver
75. nanoparticles: a green method. Carbohydr. Res.
76. : 2627-31.
77. Wang X., Chen Y., 2008. A new two-phase
78. system for the preparation of nearly mono disperse
79. silver nanoparticles,Mater. Lett.62: 4366ââ‚‌“8.
80. Goudarzi A., MotedayenAval G., Park S. S.,
81. Choi M.C., Sahraei R., 2009. Antisolvent-induced
82. encapsulation for extraction/preconcentration of
83. silver nanoparticles,Chem. Mater. 21: 2375-85.
84. Slejko F. L., 1985. Adsorption Technology: A
85. Step by step approach to process evaluation
86. application. Marcel Dekker, NY.
87. SuffetI H., McGurie M. J., 1985. Activated
88. carbon adsorption of organics from aqueous
89. phase.Ann.Arbor. Sci. Michigan. 1ââ‚‌“2.
90. Mittal A., Kurup L., Mittal J., 2007.
91. Freundlich andLangmuir adsorption isotherms and
92. kinetics for the removal of Tartrazine from
93. aqueous solutions using hen feathers. J. Hazard
94. Mater. 146:243ââ‚‌“248.
95. Langmuir I., 1916. The constitution and
96. fundamental properties of solids and liquids. J.
97. Am. Chem. Soc. 38:2221ââ‚‌“2295.
98. Crini G., 2006. Non-conventional low-cost
99. adsorbents for dye removal, a review.Bioresour.
100. Technol. 97:1061ââ‚‌“1085.
101. Temkin M. J., Pyzhev V., 1940. Recent
102. modification to Langmiur
103. isotherms.ActaPhysiochim. USSR. 12: 217ââ‚‌“222.
104. Rengaraj S., KimY., Joo C. K., Yi J., 2004.
105. Removal of copper from aqueous solution by
106. aminated and protonated mesoporousaluminas:
107. kinetics and equilibrium. J. Colloid Interf. Sci.
108. :14-21.
109. Sari A., Tuzen M., 2008. Biosorption of
110. cadmium (II) from aqueous solution by red algae
111. (Ceramiumvirgatum): Equilibrium, kinetic and
112. thermodynamic studies. J. Hazard.Mater. 157:448-