carbon.pdf
TRANSCRIPT
-
C A R B O N 4 8 ( 2 0 1 0 ) 1 0 3 2 1 0 3 7
. sc iencedi rec t .com
avai lab le at wwwjournal homepage: www.elsev ier .com/ locate /carbon
Evidence for the presence of cyanide during carbonactivation by KOH
E. Fuente a, R.R. Gil a, R.P. Giron a, M.A. Lillo-Rodenas b, M.A. Montes-Moran a,*,M.J. Martin c, A. Linares-Solano b
a Instituto Nacional del Carbon, CSIC, Apartado 73, E-33080 Oviedo, Spainb Grupo de Materiales Carbonosos y Medioambiente (MCMA), Departamento de Qumica Inorganica, Universidad de Alicante,
Apartado 99, E-03080 Alicante, Spainc Labotarori dEnginyeria Qumica i Ambiental (LEQUIA), Institut de Medi Ambient, Facultat de Ciencies, Universitat de Girona,
17071 Girona, Spain
A R T I C L E I N F O
Article history:
Received 27 July 2009
Accepted 9 November 2009
Available online 12 November 2009
0008-6223/$ - see front matter 2009 Elsevidoi:10.1016/j.carbon.2009.11.022
* Corresponding author: Fax: +34 985 297662.E-mail address: [email protected] (M.A
A B S T R A C T
The observation that carbon activation by KOH gives rise to a significant formation of cya-
nide moieties is confirmed. However, contrary to what has been reported, our results show
that the N2 used as an atmosphere during the activation process has little to do with the
formation of such cyanide moieties. The main source of cyanides is ascribed to structural
nitrogen already present in the precursors. Reducing species (H2 and metallic K) formed
during the KOH carbon activation process might promote the transformation of that struc-
tural nitrogen to cyanides. In order to minimise cyanide formation (and related environ-
mental concerns), materials with low nitrogen content should be selected as precursors
for the preparation of KOH-activated carbons.
2009 Elsevier Ltd. All rights reserved.
1. Introduction
Research carried out using alkaline hydroxides as activating
agents for different carbon precursors has been profusely re-
ported. NaOH and KOH activation makes possible activated
carbons with rather unique textural properties, i.e., extremely
high apparent specific surface areas (SBET values as high as
4000 m2 g1 being eventually claimed) and pore volumes.
Thus, chemical activation with hydroxides has become a
recognised method to obtain the sometimes referred to as
super activated carbons [18].
The growing interest on alkaline activation has also
prompted several studies to better understand the mecha-
nism involved. It is now well-established that different chem-
ical pathways occur depending on the nature of the precursor,
raw materials (i.e., lignocellulosic materials) on one side [9],
and carbonaceous precursors (chars, coals, etc.) on the other
er Ltd. All rights reserved. Montes-Moran).
[1,1012]. For this latter type of carbon precursors, the follow-
ing redox mechanism has been proposed from the reaction
products observed during activation performed at tempera-
tures around 750 C [1,1012]:
6MOH 2C! 2M2CO3 2M 3H2 1
M being K or Na. This chemical reaction accounts for the C
oxidation that should develop the porous network in the
remaining carbon material.
In principle, chemical reactions involving other elements
than C (heteroatoms) should be also prone to occur during
the activation, as far as they are present in the precursor. Re-
search contributions on the possible evolution of those other
elements during alkaline activation are scarce, apart from the
interesting recent work of Robau-Sanchez et al. [13,14] where
evidence of cyanide formation during the KOH activation of a
Quercus agrifolia char has been reported. These authors found
.
http://dx.doi.org/10.1016/j.carbon.2009.11.022mailto:[email protected]://www.elsevier.com/locate/carbon -
C A R B O N 4 8 ( 2 0 1 0 ) 1 0 3 2 1 0 3 7 1033
that considerably more cyanide was formed under nitrogen
than under argon, leading to the conclusion that cyanide
was produced mainly from N2. These unexpected results are
very surprising in view of the kinetic stability of dinitrogen.
Additionally, they are not in agreement with what was re-
ported in Refs. [1,15], where the effect of the type of gas used
during alkaline activations on the textural properties of the
activated materials was analysed. It was concluded that,
independently of the nature of the gas used (He, Ar or N2),
they only work as purging gases, displacing the global chem-
ical activation reaction towards the products.
In a series of recent contributions, using alkaline hydrox-
ide activation of sludge-based precursors [1619], cyanide
moieties were detected in the activated materials [17,19],
which confirms the results of Robau-Sanchez et al. [13,14].
Such confirmed cyanide formation requires further studies
because of its importance for environmental protection.
Thus, the aim of the present paper is to delve into the causes
of the cyanide formation. For that purpose, precursors with
different nitrogen contents have been selected to address
the contribution of the two possible N sources to cyanide for-
mation: structural nitrogen, or nitrogen coming from the
flowing gas as suggested by Robau-Sanchez et al. [13,14].
2. Experimental
2.1. KOH activation
Chars were prepared from selected residues attending to
their nitrogen content: a lignocellulosic (Quercus Robur) saw
dust (QUE), two chromium-free solid wastes from the leather
industry (CUA and CUB) and two sewage sludges (SB and
BIOS) collected at two different Spanish wastewater treat-
ment plants (WWTP). SB sludge has been used in previous
works ([1619]). The BIOS sludge was collected directly from
the aeration tank of the activated sludge unit (Girona
WWTP).
Char precursors were obtained from the pyrolysis of the
abovementioned residues for their subsequent activation pro-
cess study. Approx. 20 g of dried residue were put into an alu-
mina crucible and placed in a ceramic tubular furnace (55 mm
i.d.). The residue was heated up to 750 C in 150 ml min1 offlowing nitrogen, using a heating rate of 5 C min1. The max-imum temperature was held for 60 min. Then, the samples
were allowed to cool down to room temperature in the same
atmosphere (N2). Precursors (chars) were finally ground and
sieved to obtain a particle size smaller than 212 lm, before
proceeding to their chemical activation. Nomenclature used
for the chars is the same as that used for their precursors
adding, at the end, -P.
Powdered KOH (Aldrich) was selected as activating agent.
Approx. 15 g of KOH/precursor mixtures prepared using vari-
ous weight ratios were placed into an alumina crucible and
heated up to 750 C, using 5 C min1 heating rate and 1 h ofdwelling in the same horizontal furnace used for pyrolysis.
The activation process was carried out in N2 or Ar at different
flow rates.
The analysis of major elements (C, H, N, S and O) of
solid samples was performed as described elsewhere [16].
The oxygen content determination corresponds to the total
content, i.e., including the metal oxides (ash).
2.2. Cyanide analysis
Six grams of the activated mixtures were split in two parts,
for duplicate analysis. Each part weighing 3 g was washed
with 80 ml of deionised water (MilliQ) in four (20 ml) succes-sive stages, at room temperature. The supernatant liquid was
collected by centrifugation of the solid suspensions. The four
aqueous solutions obtained in every washing plus centrifuga-
tion step were finally mixed. pH of the aqueous solutions
were measured using a TIM870 titration system from
Radiometer.
Total cyanide contents of the two duplicate solutions per
sample (80 ml each) were quantified combining the US EPA
9014 [20] and 9010C methods [21]. Basically, cyanides are re-
leased from the aqueous solutions as hydrocyanic acid
(HCN), by means of a reflux-distillation operation under acidic
conditions, and absorbed in a scrubber containing sodium
hydroxide solution. Interferences are mostly eliminated
by using this distillation procedure [21]. The cyanide concen-
tration in the absorbing solution was then determined [20]
using a UV 2401PC UVvis recording spectrophotometer
(Shimadzu).
3. Results and discussion
The elemental compositions of the five selected residues and
their corresponding chars are collected in Table 1. As men-
tioned in the experimental section, the N content of the dif-
ferent residues spans a relatively wide range of values, from
less than 1% for the lignocellulosic residue QUE to more than
10% for the CUA sample. In terms of their inorganic (ash) con-
tent, the residues could be grouped in two sets, with the QUE
and CU* samples (especially CUA) having very low ash con-
tents and the sludges having relatively high contents (around
30%). After pyrolysis, the initial range of N contents shortens,
especially if daf values are considered. The nitrogen content
in the pyrolysed samples (precursors) is assumed to be linked
to the carbon-rich (char) fraction of the materials, since any
inorganic nitrogen species in the original residues should
not withstand the thermal treatment.
It is confirmed, in agreement with Refs. [13,14,17,19] that
cyanide species were produced in all activation experiments,
regardless of the precursor and conditions employed. They
were analysed indirectly by washing the activated mixtures
using water at room temperature. Preliminary tests (results
not shown) allowed us to conclude that four washing steps
(as described in Section 2) were enough to virtually attain
the complete transfer of the different cyanide moieties,
mainly KCN, to the aqueous solutions. Table 2 shows the cya-
nide concentration of the solutions obtained when washing
activated mixtures prepared using 1/1 KOH/precursor weight
ratios, under nitrogen. The repeatability of the washing pro-
cedure within a given sample was excellent in all cases.
Henceforth, for each activation experiment, only average con-
centration values obtained from the two measurements will
be reported. For two of the samples, namely CUA-P and
-
QUE-P
CUA-P
CUB-P
SB-P
BIOS-P
0 20 40 60 80 100 120[CN- ] (mg g-1)
Ar N2
Fig. 1 Comparison between the amount of cyanides
obtained during the activation of the different precursors
under N2 and Ar.
Table 1 Elemental analysis (dry basis) of the residues and corresponding chars.
Sample Ash content Elemental analysis (wt.%)
(wt.%) C H N S O
QUE
-
150/1
150/3
500/3
0 10 20 30 40[CN- ] (mg g-1)
Ar N2
Fig. 3 Cyanide formation in the course of the activation of
SB-P using different KOH/precursor ratios and flow rates,
under N2 and Ar.
C A R B O N 4 8 ( 2 0 1 0 ) 1 0 3 2 1 0 3 7 1035
Other important issue that should be addressed when
dealing with alkaline hydroxide activation of carbons is the
effect of both nitrogen flow rate and the KOH/precursor ratio.
Two of the precursors under study, namely SB-P and CUB-P,
were selected to carry out additional experiments using dif-
ferent activation conditions. Labelling of the new samples
obeys the following rationale: A/B, A being the flow rate (in
ml min1) and B being the KOH/precursor weight ratio. Re-
sults are shown in Figs. 2 and 3.
Figs. 2 and 3 confirm that the precursor with higher nitro-
gen content leads to higher cyanide amounts and that both
char precursors behave similarly. Although differences are
not very pronounced, it seems that an increase in the carrier
gas flow rate or in the relative proportion of the activating
agent produces, interestingly, solutions with a higher concen-
tration of cyanides. This observation has not been reported
before, as far as Robau-Sanchez et al. failed to find any rela-
tionship between the activation conditions and the amount
of cyanides detected [13].
A nitrogen mass balance study was carried out to better
understand the effect of the activating conditions on the for-
mation of cyanides. Elemental analyses of the water-washed
samples were carried out to determine the nitrogen remain-
ing in the activated solids after cyanide removal. Results are
shown in Table 3, keeping a constant basis for the calcula-
tions (100 g of precursor). The increase of the CN concentra-
tion in the aqueous solutions obtained when activation is
carried out at higher flow rates or KOH/precursor ratios (Figs.
2 and 3, and NL values in Table 3) are attained at the expense
of the nitrogen remaining in the washed solids, so to keep the
amount (Ns,f + NL) relatively constant for a given precursor,
regardless of the activation conditions.
Having more CN transferred from the activated solids to
the aqueous solution when the activation is carried out under
higher flow rates or activating agent/precursor ratios could be
due not only to the formation of cyanide species during the
process. It might be also a consequence of an eventual change
in the solubility conditions of the cyanide salts. The similarity
between the pH values of the solutions obtained from a given
precursor activated in Ar and in N2 under different conditions
150/1
500/1
150/3
500/3
0 20 40 60 80 100[CN- ] (mg g-1)
Ar N2
Fig. 2 Cyanide formation in the course of the activation of
CUB-P using different KOH/precursor ratios and flow rates,
under N2 and Ar.
(Table 3) rules out this possibility. Thus, the increment of the
cyanide concentration in the aqueous solutions measured at
higher flow rates or KOH/precursor ratios is most likely linked
to the completion of a chemical reaction involving the forma-
tion of cyanides during the activation. This increase in the
cyanide amount detected in these experiments is consistent
and must be related to a higher activation degree [13].
All the above results indicate that cyanides, ascribed to
structural nitrogen already present in the precursors, are
formed during the activation reaction, as XRD analysis of
the solids obtained after activation (i.e., before being washed)
confirms [19]. These cyanides are produced as a consequence
of the reducing atmosphere formed during the KOH carbon
activation process. Thus, when heating the carbon precur-
sor/KOH mixture in an inert atmosphere, usually in the tem-
perature range of 750850 C, carbon oxidation (carbonconversion to potassium carbonate) takes place, together
with the formation of reducing products (metallic K and H2),
responsible of cyanide formation.
The cyanide concentrations reported by Robau-Sanchez
et al., when activating a lignocellulosic char in N2 (i.e., approx.
300 mg g1) [13], are two orders of magnitude higher than
those obtained for the QUE-P sample (Table 2, Fig. 1). Compo-
sitional differences between the two lignocellulosic chars un-
der consideration (see Table 2 in [13] and Table 1 above)
cannot justify such a significant variation in the amount of
cyanides detected. A possible explanation is that they em-
ployed a stainless steel reactor (in the present work an alu-
mina crucible) where the char/KOH mixtures were placed in
direct contact with the reactor wall. Fe has been traditionally
used as catalyst in the production of alkaline cyanides from
gaseous N2 [22,23]. The nitrogen mass balances of Table 3 ex-
cludes N2 fixation, within experimental error (DN = 0 1).
Fig. 4 shows a clear dependence of the amount of CN de-
tected in the liquid phase on Ns,0 (see Table 3), for activations
carried out under the same experimental conditions (i.e.,
100 g of precursor, 1:1 KOH:precursor ratio) and 150 ml min1 of Ar or N2. The trend depicted in Fig. 4 can be fairly ac-
cepted to be valid for precursors whose inorganic fraction
does not promote N2 fixation (a significant presence of transi-
tion metals, for example). Nevertheless, in that case, impor-
-
Table 3 Nitrogen mass balances of the activation process.
Precursor Conditionsa NS,0b NS,f
c NLd DNe pH
QUE-P N2/150/1 0.8 0.6 0.18 0.0 13.08Ar/150/1 0.7 0.10 0.0 12.99
CUA-P N2/150/1 8.9 2.0 6.91 0.0 12.83Ar/150/1 2.4 6.52 0.0 12.82
CUB-P N2/150/1 6.0 2.1 3.91 0.0 12.78Ar/150/1 1.9 3.93 0.3 12.78N2/150/3 1.0 4.40 0.6 12.49Ar/150/3 0.8 4.65 0.6 12.45N2/500/1 1.5 4.13 0.4 12.75Ar/500/1 1.2 4.57 0.3 12.76N2/500/3 0.5 4.85 0.6 12.59Ar/500/3 0.4 5.24 0.4 12.60
SB-P N2/150/1 2.6 1.0 1.51 0.1 13.09Ar/150/1 1.0 1.52 0.1 13.07N2/150/3 0.8 1.57 0.2 13.02Ar/150/3 0.8 1.67 0.1 12.95N2/500/3 0.5 1.99 0.4 13.07Ar/500/3 0.5 1.85 0.2 13.07
BIOS-P N2/150/1 3.1 1.6 0.96 0.5 12.79Ar/150/1 1.4 1.26 0.4 12.81
a Activation atmosphere/flow rate/KOH/precursor ratio.b Gram of N in 100 g of the precursor.c Gram of N in the washed, activated samples obtained from 100 g of the precursor.d Gram of N in the washing solutions (from total CN content) of activated samples obtained from 100 g of the precursor.e N balance: NS,0 (NS,f + NL).
0 2 4 6 8 100
2
4
6
8
10
12
14
CN
- (g)
NS,0 (g)
N2 Ar (R2 = 0.94)
Fig. 4 Dependence of the amount of cyanides detected on
NS,0 (Table 3) during the activation of the different
precursors under the same experimental conditions (100 g
of precursor, 1:1 KOH:precursor ratio) and 150 ml min1 of
Ar or N2.
1036 C A R B O N 4 8 ( 2 0 1 0 ) 1 0 3 2 1 0 3 7
tant differences in the amount of cyanides formed under
nitrogen or argon should be expected.
4. Conclusions
Soluble cyanide is formed during the alkaline activation of
nitrogen-containing chars as a consequence of structural
nitrogen present in the precursor. The amount of cyanides ob-
tained when the activation is carried out under nitrogen or ar-
gon atmospheres is essentially the same, as far as iron or
other cyanide formation promoters are absent from the reac-
tion chamber. Increasing the flow rate or KOH/precursor ratio
tends to raise the amount of cyanides formed. A correlation
between the cyanides detected in solution and the nitrogen
content of the precursors could be established. Cyanide for-
mation during chemical activation with hydroxides can be
minimised by reducing the N content of the precursor. Finally,
attention should be paid to the KOH activation process of
some carbon precursors because high cyanide concentrations
(e.g., as high as 130 mg of CN per gram of precursor) can be
eventually reached for chars with relatively high N contents
(e.g., 9 wt.%, dry basis). This remarks that materials with
low nitrogen content should be selected, from an environ-
mental point of view, to be used as precursors for the prepa-
ration of activated carbons by KOH activation.
Acknowledgements
This work was funded by MEC and MICINN (CTM2005-07524-
C02-00, CTM2008-06869-C02-00/PPQ and PRT2007-0421
projects).
R E F E R E N C E S
[1] Linares-Solano A, Lozano-Castello D, Lillo-Rodenas MA,Cazorla-Amoros D. Carbon activation by alkaline hydroxides:preparation and reactions, porosity and performance. In:Thrower PA, editor. Chemistry and physics of carbon, vol.30. Boca Raton: CRC Press; 2008. p. 162.
-
C A R B O N 4 8 ( 2 0 1 0 ) 1 0 3 2 1 0 3 7 1037
[2] Lozano-Castello D, Lillo-Rodenas MA, Cazorla-Amoros D,Linares-Solano A. Preparation of activated carbons fromSpanish anthracite: I. Activation by KOH. Carbon2001;39(5):7419.
[3] Lillo-Rodenas MA, Lozano-Castello D, Cazorla-Amoros D,Linares-Solano A. Preparation of activated carbons fromSpanish anthracite: II. Activation by NaOH. Carbon2001;39(5):7519.
[4] Ahmadpour A, Do DD. The preparation of activated carbonfrom macadamia nutshell by chemical activation. Carbon1997;35(12):172332.
[5] Otowa T, Nojima Y, Miyazaki T. Development of KOHactivated high surface area carbon and its application todrinking water purification. Carbon 1997;35(9):13159.
[6] Perrin A, Celzard A, Albiniak A, Kaczmarczyk J, Mareche JF,Furdin G. NaOH activation of anthracites: effect oftemperature on pore textures and methane storage ability.Carbon 2005;43(9):19909.
[7] Tian HY, Buckley CE, Wang SB, Zhou MF. Enhanced hydrogenstorage capacity in carbon aerogels treated with KOH. Carbon2009;47(8):212830.
[8] Teng H, Hsu L-Y. High-porosity carbons prepared frombituminous coal with potassium hydroxide activation. IndEng Chem Res 1999;38(8):294753.
[9] Daz-Teran J, Nevskaia DM, Fierro JLG, Lopez-Peinado AJ, JerezA. Study of chemical activation process of a lignocellulosicmaterial with KOH by XPS and XRD. Micropor Mesopor Mater2003;60(13):17381.
[10] Lillo-Rodenas MA, Juan-Juan J, Cazorla-Amoros D, Linares-Solano A. About reactions occurring during chemicalactivation with hydroxides. Carbon 2004;42(7):13715.
[11] Lillo-Rodenas MA, Cazorla-Amoros D, Linares-Solano A.Understanding chemical reactions between carbons andNaOH and KOH: an insight into the chemical activationmechanism. Carbon 2003;41(2):26775.
[12] Raymundo-Pinero E, Aza P, Cacciaguerra T, Cazorla-AmorosD, Linares-Solano A, Beguin F. KOH and NaOH activationmechanisms of multiwalled carbon nanotubes with differentstructural organisation. Carbon 2005;43(4):78695.
[13] Robau-Sanchez A, Aguilar-Elguezabal A, Aguilar-Pliego J.Chemical activation of Quercus agrifolia char using KOH:evidence of cyanide presence. Micropor Mesopor Mater2005;85(3):3319.
[14] Robau-Sanchez A, Cordero-de la Rosa F, Aguilar-Pliego J,Aguilar-Elguezabal A. On the reaction mechanism of thechemical activation of Quercus agrifolia char by alkalinehydroxides. J Porous Mater 2006;13:12332.
[15] Lillo-Rodenas MA, Juan-Juan J, Cazorla-Amoros D, Linares-Solano A. Further comments about the reactions occurringduring carbon activation with hydroxides. In: Proceedings ofCARBON 2005 International Conference, July 37 2005.Gyeongju, Korea: Korean Carbon Society; 2005.
[16] Ros A, Lillo-Rodenas MA, Fuente E, Montes-Moran MA,Martin MJ, Linares-Solano A. High surface area materialsprepared from sewage sludge-based precursors.Chemosphere 2006;65:13240.
[17] Ros A, Lillo-Rodenas MA, Canals-Batlle C, Fuente E, Montes-Moran MA, Martin MJ, et al. A new generation of sludge-based adsorbents for H2S abatement at room temperature.Environ Sci Technol 2007;41:437581.
[18] Canals-Batlle C, Ros A, Lillo-Rodenas MA, Fuente E, Montes-Moran MA, Martin MJ, et al. Carbonaceous adsorbents forNH3 removal at room temperature. Carbon 2008;46:1768.
[19] Lillo-Rodenas MA, Ros A, Fuente E, Montes-Moran MA,Martin MJ, Linares-Solano A. Further insights into theactivation process of sewage sludge-based precursors byalkaline hydroxides. Chem Eng J 2008;142:16874.
[20] US EPA. Titrimetric and manual spectrophotometricdeterminative methods for cyanide. In: Test methods forevaluating solid waste (SW-846), CD-ROM; 1996. p. 9014-17.
[21] US EPA. Total and amenable cyanide: distillation. In: Testmethods for evaluating solid waste (SW-846), CD-ROM; 2004.p. 9010C-110.
[22] Bucher JE. The fixation of nitrogen. Ind Eng Chem1917;9:23353.
[23] Babor JA, Ibarz J. Qumica General Moderna. 7th ed. Madrid,Spain: Marn SA; 1968. p. 7034.
Evidence for the presence of cyanide during carbon activation by KOHIntroductionExperimentalKOH activationCyanide analysisResults and discussionConclusionsAcknowledgementsReferences