Sulfurization of a carbon surface for vapor phase mercury removal – II: Sulfur forms and mercury uptake

Feng, Wenguo; Borguet, Eric; Vidic, Radisav D.

doi:10.1016/j.carbon.2006.05.053

Cited by 130 publications

(103 citation statements)

References 23 publications

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“…Sulfur impregnation has been shown to significantly enhance the Hg 0 adsorption of activated carbons [2][3][4][5][6][7][8][9][10][11]. Our earlier works also indicated that activated carbons with greater Hg adsorption can be developed by treating them with elemental sulfur at temperatures between 200 and 650°C [6,7].…”

Section: Introductionmentioning

confidence: 85%

Influences of acidic/oxidizing gases on elemental mercury adsorption equilibrium and kinetics of sulfur-impregnated activated carbon

Hsi

Chen

2012

Fuel

119

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Section: Introductionmentioning

confidence: 85%

Influences of acidic/oxidizing gases on elemental mercury adsorption equilibrium and kinetics of sulfur-impregnated activated carbon

Hsi

Chen

2012

Fuel

119

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“…Surface chemical modification of adsorbents with the aim of promoting their ion exchange properties for stronger and selective adsorption of special compounds has attained great interest recently (Krishnan and Anirudhan 2008;Nam et al 2003;Rios et al 2003;Lee et al 2004; Mersorb ® Mercury adsorbents 2010). Previous studies have shown that introducing sulfur functionalities onto the surface of adsorbents can improve their mercury uptake capacity (Feng et al 2006;Hsi et al 2002;Wajima et al 2009). This idea is inspired by Pearson rule; according to this theory, oxygen molecules which naturally exist on the surface of typical activated carbons are hard bases and react hardly with metal ions such as Hg 2+ (soft acid).…”

Section: Introductionmentioning

confidence: 98%

A comparison on efficiency of virgin and sulfurized agro-based adsorbents for mercury removal from aqueous systems

Asasian

Kaghazchi

2012

Adsorption

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Mercury adsorption by sulfur impregnated adsorbents seems to be one of the most efficient ways for removal of this toxic metal ion from wastewater and atmosphere. The aim of this work was to develop a method for preparation of low-cost sulfurized adsorbent from agricultural wastes; this approach combines two stages of (i) chemical activation with phosphoric acid and (ii) impregnation with powdered sulfur, in one step only. The physico-chemical properties of sulfurized adsorbent (AC-S) were determined with BET, FT-IR, Eschka method and pH PZC measurements, and compared with those of the virgin sample (AC). It was found that sulfurization according to this method can introduce about 8 wt.% sulfur into the structure of adsorbent, in the forms of C-S, S-H, S-S and S=O functional groups. Although during the sulfur introduction processes, a decrease in surface area and micropore volume of the sulfurized adsorbent is to be expected, not only such decrease did not occur in this work, but a large increase in microporosity was seen. Thereupon, both the sulfur functionalities and extended microporosity of AC-S lead to higher capability of this sample for mercury adsorption rather than AC. Finally, the kinetics and equilibrium of mercury adsorption from aqueous solutions were studied for AC and AC-S. Nomenclature BConstant of D-R isotherm related to energy, (mol 2 /J 2 ) C 0 the solute concentration at time t = 0, (mg/l) C t the solute concentration at time t, (mg/l) C e the solute concentration at equilibrium, (mg/l) [in D-R model (g/g)] ePolanyi potential in D-R model E Free energy of adsorption, (J/mol) h (= k 2 q 2 e ) the initial sorption rate, (mg/g min) k 1 Pseudo-first-order adsorption rate constant, (1/min) k 2 Pseudo-second-order adsorption rate constant, (g/mg min) K F Freundlich empirical constant, (mg/g)(mg/l) −1/n K L Langmuir empirical constant (l/mg) K T Equilibrium binding constant corresponding the maximum binding energy, (l/mg) n the exponent in Freundlich isotherm N the number of runs p the number of model's parameters q i,exp the amount of solute adsorbed on the adsorbent observed from the ith run of experiment, (mg/g) q i,calc the amount of solute adsorbed on the adsorbent estimated from the model for corresponding q i,exp , (mg/g) q t the amount of solute adsorbed at time t, (mg/g) q e the amount of solute adsorbed at equilibrium, (mg/g) [in D-R model (mol/g)] q m Monolayer adsorption capacity (in Langmuir model (mg/g)), (in D-R model the theoretical monolayer saturation capacity (mol/g)) RUniversal gas constant, (8.313 J/mol K) R 2 Correlation coefficient RMSE Root mean squared error function t Time, (min) 190 Adsorption (

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“…At room temperature, H 2 S adsorbs on coke through both physical and chemical mechanism [12,13]. At high temperatures, chemical adsorption dominates and resulting in the formation of sulfurcontaining species in the coke [14][15][16]. Our early study showed that H 2 S reacts with a coke (with an ash content of 0.85%) at temperatures from 200 to 800 8C and results in an increase in the sulfur content of coke [17].…”

Section: Introductionmentioning

confidence: 99%

Influence of silicon on uptake of H2S by a coke under elevated temperature

Zhou¹,

Yang²,

Liu³

et al. 2009

Journal of Analytical and Applied Pyrolysis

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Sulfurization of a carbon surface for vapor phase mercury removal – II: Sulfur forms and mercury uptake

Cited by 130 publications

References 23 publications

Influences of acidic/oxidizing gases on elemental mercury adsorption equilibrium and kinetics of sulfur-impregnated activated carbon

Influences of acidic/oxidizing gases on elemental mercury adsorption equilibrium and kinetics of sulfur-impregnated activated carbon

A comparison on efficiency of virgin and sulfurized agro-based adsorbents for mercury removal from aqueous systems

Influence of silicon on uptake of H2S by a coke under elevated temperature

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