Open Access

Structural Features of Carbons Produced Using Glucose, Lactose, and Saccharose

  • Ivan F. Myronyuk1,
  • Volodymyr I. Mandzyuk1Email author,
  • Volodymyr M. Sachko1 and
  • Volodymyr M. Gun’ko2
Nanoscale Research Letters201611:508

Received: 20 October 2016

Accepted: 4 November 2016

Published: 17 November 2016


Glucose, lactose, and saccharose were used as precursors to prepare chars at 400 °C then activated at 800 °C or 1000 °C in closed vessels with controlled amounts of oxygen penetrating through nanopores in the vessel walls. There are correlations between the porosity, amounts of residual O- and H-containing functionalities, and electroconductivity of amorphous carbons studied. The pore size distributions calculated using the nitrogen adsorption isotherms and TEM images show that all carbons are mainly nanoporous with certain contribution of narrow mesopores (at pore half-width x < 5 nm). Oxidizing activation by oxygen penetrating into the closed vessels with chars through nanopores can more strongly change the outer layers of char particles than the inner pores. Therefore, despite relatively great burn-off degree, the textural characteristics are relatively low for activated carbons.


Activated carbons Thermal degradation processes Porous structure, surface functional groups Specific conductivity


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Carbons are frequently produced using natural row materials, which include carbohydrates [113]. Carbohydrates (e.g., saccharides) are appropriate materials for carbonization because they include many well-removed O/H-containing functionalities [1425]. Therefore, their carbonization with the dehydration as one of the main processes can be carried out at temperatures (320–500 °C) lower than that used for carbonization of other compounds, e.g., phenolformaldehyde resin at 800 °C [2628]. To improve the textural characteristics of chars, they are activated in the atmosphere with water vapor, CO2, or CO at 800–1100 °C [13, 29]. Carbonization of precursors mixed with such active compounds as zinc chloride, phosphorus acid, and potassium carbonate can provide a high porosity of the carbons without of additional activation [3032].

The physicochemical properties of the carbonaceous materials depend strongly on the characteristics of their precursors. Since chars are composed of polyaromatic structures (graphenes), the presence of cyclic fragments in the precursors is favorable for effective carbonization. Therefore, thermolysis of mono- or disaccharides results in the formation of polyaromatic compounds, whose condensation gives graphene clusters. Among simple carbohydrates, saccharose is frequently used as a char precursor [1325, 3335]. Mono- and disaccharides are characterized by tautomerism and diastereoisomerism, e.g., besides chain-cyclic tautomerism of glucose, there are eight pairs of its diastereomers. The tautomers and diastereomers (stereoisomers not related as mirror images) are characterized by different physicochemical properties [36, 37]. This can affect the carbonization results for saccharides. Note that carbonization of glucose or other small organic molecules at a surface of oxide materials (such as silica gels, fumed silica, titania, and mixed oxides) typically results in the formation of nonporous carbon nanoparticles similar to those of carbon black [38, 39]. Besides dependences of the textural characteristics of chars on the structure of different saccharides used as precursors, there is an additional question on the effects of activation of chars by small controlled portions of oxygen. Therefore, the aim of this work was to study the thermolysis of glucose (as a monosaccharide) and two disaccharides (such as lactose composed of β-d-galactopyranose and α-d-glucopyranose and saccharose composed of α-d-glucopyranose and β-d-fructofuranose), and the characteristics of the chars (carbonized at 400 °C) and related carbons activated at 800 and 1000 °C using controlled amounts of oxygen.


Crystalline monohydrates of glucose, lactose, and anhydrous saccharose were used as precursors of chars prepared at 400 °C for 30 min in air. Oxidizing activation of chars was carried out in ceramic crucibles at 800 or 1000 °C for 30 min. Oxygen (from air) penetrated into the crucibles through mesoporous walls (porosity ~20%). The pore sizes in the walls were decreased by fourfold to fivefold impregnation with a concentrated solution of AlONO3 2H2O, dried, and then calcined at 800 °C. Mesoporous alumina filling macropores of the crucible walls has pores of approximately 5 nm in size. Caps of the crucibles were sealed using asbestos strings.

Thermal degradation of glucose, lactose, and saccharose in 25–1000 °C range was studied using thermogravimetry (TG) with a STA 449 F3 Jupiter (Netzsch) apparatus at a heating rate of 5 °C/min in the inert (argon) atmosphere.

The textural characteristics of chars and activated carbons, AC (degassed at 180 °C for 24 h), have been determined using the nitrogen adsorption-desorption isotherms recorded at 77.4 K using a Quantachrome Autosorb Nova 2200e adsorption analyzer. The pore size distributions (PSDs) (differential ~ dV/dx) have been calculated using the quenched solid density functional theory (QSDFT, Quantachrome software) [40] and 2D-nonlocal DFT (2D-NLDFT, SAIEUS program, Micromeritics software) [41, 42] methods with the slit-shaped pore model. Additionally, the complex model with slit-shaped (S) and cylindrical (C) pores and voids (V) between nanoparticles (SCV-model) with self-consisting regularization (SCR) procedure was used [43]. The differential PSD functions with respect to the pore volume (PSDV, f V(x) ~ dV/dx, ∫f V(x)dx ~ V p) and the specific surface area (PSDS, f S(x) ~ dS/dx, ∫f S(x)dx ~ S) were used to estimate the contribution of nano- (x < 1 nm), meso- (1 < x < 25 nm), and macropores (x > 25 nm).

The X-ray diffraction (XRD) patterns of samples treated at different temperatures were recorded at room temperature using a DRON-4-07 (Burevestnik, St. Petersburg) diffractometer with Cu Kα (λ = 0.154178 nm) radiation and a Ni filter in the 2θ range from 10° to 65° with a step of 0.1° using the Bragg-Brentano geometry.

Infrared (IR) spectra were recorded using a Specord M80 spectrometer over the 400–4000 cm−1 range. A sample (4 mg) was stirred with dry KBr (weight ratio 1:100), treated in a stainless steel microbreaker for 10 min, and pressed in a thin transparent plate of 20 × 5 mm2 in size.

Transmission electron microscopy (TEM) images have been obtained using a JEOL JSM-2100F field emission TEM operated at 200 kV. TEM images have been analyzed using Fiji (local thickness plugin) [44] and ImageJ (granulometry plugin) [45, 46] software.

Desorption of fragments with C4, C5, C6, and C9, as well as CO, CO2, and others, was analyzed using temperature-programmed desorption (TPD) with mass-spectroscopic (MS) control using a MX 7304A mass spectrometer (Electron, Sumy, Ukraine, sensitivity ~10−8 g at m/z 1–400) [47, 48]. A sample (4 mg) placed in a quartz–molybdenum cell (diameter 11 mm) was degassed at room temperature and pressure 7 × 10−5 Pa and then heated to 800 °C at a linear heating rate of 1 °C/min. Volatile products are desorbed from the sample, ionized by the electron beam, separated by a mass-analyzer, and brought to a detector.

Impedance analysis of carbon samples was carried out using a Metrohm Autolab FRA-2 (Frequency Response Analyzer) at 10−2–105 Hz and voltage amplitude of 10 mV [49].

Results and Discussion

The thermolysis of glucose, lactose, and saccharose in the inert atmosphere (Fig. 1, Table 1) shows several processes: desorption of intact water (65–145 °C for glucose and 100–175 °C for lactose as crystalline hydrates), melting, caramelization, dehydration (associative desorption of water molecules), carbonization (formation of polyaromatics and carbon sheets and graphenes), and structure transformation of chars.
Fig. 1

Saccharide thermolysis corresponding to mass loss (thermogravimetry (TG)), differential TG (DTG), and differential thermal analysis (DTA) curves for a glucose, b lactose, and c saccharose

Table 1

Processes observed during heating of precursors to 1000 °C








Intact water removal

 Temperature (°C)



 Water loss (mole)




 Temperature (°C)





 Temperature (°C)




 Water loss (mole)





 Temperature (°C)




 Water loss (mole)




 Residual mass (%)




Char structure changes

 Temperature (°C)




 Residual mass (%)




 Mass loss in this process (%)




The maximal rate of removal of intact water is at 96 °C for glucose and 144 °C for lactose (Fig. 1a, b, DTG). The processes of water removal, caramelization (~160 °C), melting (160, 220, and 197 °C for glucose, lactose, and saccharose, respectively), and dehydration are endothermic ones (Fig. 1, DTA minima). Removal of water due to the condensation reactions between the hydroxyl groups of interacting molecules and the formation of polyaromatic compounds occur at 200–330 °C (glucose), 230–355 °C (lactose), and 218–345 °C (saccharose). These processes result in the mass loss (Table 1). The residual mass corresponds to 40% (glucose and lactose) and 42% (saccharose) with respect to the initial precursor mass. This corresponds to the loss of a major fraction of structural water due to condensation of O-containing functionalities. Subsequent heating to 1000 °C leads to the mass loss up to 88% (saccharose), 84.3% (glucose), and 82.9% (lactose). Residual carbon remains because the process was carried out in the inert atmosphere.

The most intensive lines in the TPDMS thermograms of chars correspond to the elimination of CO and CO2 (Fig. 2). This suggests that the residual amounts of O-containing functionalities in the chars are relatively great. Certain amounts of H-containing functionalities should be remained in the chars. These results are in agreement with the IR spectra of L400 (Fig. 3) showing the presence both C–H (bands at 2924–2916 and 2868 cm−1) and O–H (a broad band at 3450 cm−1) functionalities in the chars. The maximal amounts of desorbed fragments (such as C4H2O at m/z 66, C5HO2 or C6H5O at m/z 93, and C6H6O2 or C9H2 at m/z 110) are observed at ~300 °C (mainly in the range of 200–500 °C, Fig. 2). However, CO elimination is maximal at 600–800 °C that corresponds to structural changes in the chars observed in the TG/DTG/DTA thermograms at high temperatures (Fig. 1).
Fig. 2

TPD mass-spectra of chars a G400, b L400, and c S400 with lines of fragments C4H2O (m/z 66), C5HO2 or C6H5O (m/z 93), C6H6O2 or C9H2 (m/z 110), and molecules CO2 (m/z 44) and CO (m/z 28)

Fig. 3

IR spectra of samples L400 and L1000

Carbonization of a melted precursor is accompanied by elimination of water vapor that results in boiling up of the reacted precursor. This provides the formation of pores in the chars. The chars and AC have a lamellar shape (Fig. 4b, d) with a stack thickness of 5–40 nm. Nanosized graphenes (1–5 nm in size) form a random amorphous structure of the carbons (Fig. 4a, c). The XRD patterns of lactose-based char and carbons (Fig. 5) and electron diffraction patterns (see Additional file 1: Figure S1) confirm that the materials are amorphous.
Fig. 4

TEM images of carbons (a, b) L800 (scale bar 5 and 50 nm) and (c, d) S800 (scale bar 10 and 100 nm)

Fig. 5

XRD patterns of L400, L800, and L1000

The most nitrogen adsorption-desorption isotherms of the carbons studied are characterized by open hysteresis loops (Fig. 6). This can be due to the presence of long and narrow pores with narrow necks close in size to the nitrogen molecules [50]. As a whole, all samples are nanoporous with a certain contribution of narrow mesopores (Table 2, Figs. 7 and 8, and in Additional file 1: Figure S2). Note that the G400 sample was with very low open porosity; therefore, the nitrogen adsorption isotherm was not recorded. However, this sample has certain closed porosity because the specific surface area estimated from the SAXS data corresponds to 185 m2/g (the procedure of SAXS investigation is described in detail in [51]).
Fig. 6

Nitrogen adsorption-desorption isotherms for chars (L400, S400) and AC

Table 2

Textural characteristics of chars and activated carbons


Burn-off (%)

ρ b (g/cm3)

S BET (m2/g)

V p (cm3/g)

S nano (m2/g)

S meso (m2/g)

V nano (cm3/g)

V meso (cm3/g)

S QSDFT (m2/g)

S NLDFT (m2/g)






























































































With respect to the weight of a aprecursor or a bchar, ρ b is the bulk density, cthe specific surface area was calculated using the SAXS data, and the values of S nano, V nano, S meso, and V meso were calculated using the SCV/SCR method

Fig. 7

Pore size distributions calculated using the 2D-NLDFT method with the slit-shaped pore model

Fig. 8

Pore size distributions of L800 (a) and S800 (b) calculated using the 2D-NLDFT and QSDFT methods with the slit-shaped pore model and TEM images (Fig. 6a, c) treated using Fiji (local thickness plugin) and ImageJ (granulometry plugin) software

An increase in the activation temperature from 800 to 1000 °C for lactose- and saccharose-based chars leads to the enhancement of the porosity (Table 2, V p, S BET). However, direction of changes in the PSD is opposite for these samples with increasing temperature (Fig. 7), and the effect is much smaller for saccharose-based carbons.

Note that the SCV/SCR method gives slightly broader PSD (see Additional file 1: Figure S2) than the 2D-NLDFT or QSDFT methods with the slit-shaped pore model (Figs. 7 and 8). However, the PSDs based on the TEM images (Fig. 8) show the presence of narrow mesopores similar to that of the SCV/SCR PSD. Therefore, the textural characteristics shown in Table 2 are based on the SCV/SCR results.

The XRD patterns are shown only for lactose-based carbons (Fig. 5) as representative materials (other carbons have similar XRD patterns). For L400, there is the main line at 2θ = 22° and a weak features at 43°. The second XRD reflection is much intensive for L800 (23° and 43°) and L1000 (24.2° and 43.6°). The inter-plate distances estimated from these values correspond to 0.404 and 0.199 nm (L800) and 0.367 and 0.207 nm (L1000). For graphite, these distances correspond to 0.338 and 0.202 nm [13]. Thus, increasing in the activation temperature leads to certain ordering of the carbon structure; however, it remains turbostratic [13] with increased inter-plate distances in comparison with those in graphite.

The IR spectra of lactose-based carbons (as representatives) show (Fig. 3) certain changes in the composition of the material during partial oxidizing (activation) at 1000 °C. For L400, the bands at 579, 1490, and 1600 cm−1 correspond to different vibrations of the CC bonds in the aromatic rings [5254]. For L1000, these bands shift to 594, 1555, and 1632 cm−1 that correspond to certain ordering of the structure and a decrease in the CC bond length. Some bands (1388, 667, 2349 cm−1) correspond to vibrations in CO2 [5256] bound to the carbons. For L1000, an intensive band ν 3 = 2343 cm−1 and less intensive band ν 1 = 1381 cm−1 shift toward lower wavenumbers in contrast to the band ν 2 = 672 cm−1. This corresponds certain changes in the surroundings of the mentioned structures during oxidizing activation with increasing temperature. The bands at 1712 and 782 cm−1 (L400) and 1703 and 790 cm−1 (L1000) correspond to the vibrations of the >C=O bonds (C is located in the aromatic ring). A broad band at 1121–1184 cm−1 corresponds to the C–O stretching vibrations [53, 54]. As mentioned above, there are the bands corresponding to the O–H (~3450 cm−1) and C–H (2924–2916 and 2868 cm−1) stretching vibrations of the functionalities bound to carbons. Some of them can be located in closed pores or in places poorly accessible for oxygen (similar to nitrogen molecules, Fig. 6). Therefore, they were not removed during oxidizing activation.

Char L400 is practically nonconducting (Fig. 9) because the values of both real (Z′) and imaginary (Z′′) components of the impedance (Z*) are high. The main component of the value of Z′′ is the capacitive reactance caused by the barrier capacity at the boundary of carbon particles and the capacity of particles per se [57]. The main reason of this result for L400 is incomplete carbonization to form pure carbon matter. Oxidizing activation of the char at 800or 1000 °C leads to a significant decrease in the resistance (Fig. 9), and the inductive impedance appears instead of the capacitance in the high-frequency range. This is due to a decrease in the content of surface functionalities and the formation of well-ordered carbon sheets. Calculations of real (σ′) and imaginary (σ′′) components of the complex conductivity (σ*) vs. frequency (f) show that the values of σ′ are greater by two to three orders of magnitude than that of σ′′ at f < 1 kHz. Estimation of the specific conductivity as the value of σ* at f → 0 (using the plot of σ* vs. logf) (Table 3) shows an increase in the conductivity with increasing temperature of char activation from 800 to 1000 °C because of the ordering of carbon sheets and a decrease in the content of O- and H-containing functionalities discussed above. Lactose-based carbons, which are most porous (Table 2), demonstrate a greater conductivity than other carbons (Table 3). This can be explained by a deeper treatment of the lactose-based carbons with removal of the O- and H-containing functionalities. Additionally, the DTA curve for lactose has the shape different from that for glucose and saccharose over a broad temperature range of 400–1000 °C (Fig. 1).
Fig. 9

Nyquist plots for lactose-based char (L400) and activated carbons (L800 and L1000)

Table 3

Specific conductivity (Ω−1 m−1) of activated carbons


Activation at 800 °C

Activation at 1000 °C











Thermolysis of glucose, lactose, and saccharose in the inert atmosphere results in the mass loss up to 88% (saccharose), 84.3% (glucose), and 82.9% (lactose) during heating to 1000 °C. Chars prepared at 400 °C contain different O- and H-containing functionalities, whose amounts decrease during oxidizing activation at 800 and 1000 °C. However, according to the IR spectra, certain amounts of these functionalities remain even after heating at 1000 °C in the inert atmosphere. During heating of the chars in vacuum in the TPDMS experiments, desorption of O- and H-containing fragments is maximal at ~300 °C.

Oxidizing activation of the chars with controlled amounts of oxygen penetrating into the closed vessels through nanosized pores results in an increase in the porosity and specific surface area of carbons depending on the type of the used precursors. The maximum enhanced porosity is observed for lactose-based carbon activated at 1000 °C. For saccharose-based carbon, the difference in the porosity of samples activated at 800 and 1000 °C is relatively small. For glucose-based carbon, a very strong decrease in the porosity is observed for carbon activated at 1000 °C.

All carbons have nanopores and narrow mesopores; broad mesopores and macropores are practically absent. The hysteresis loops of the nitrogen adsorption-desorption isotherms are open for all chars and carbons with one exception of lactose-based carbon L1000 activated at 1000 °C and possessing the maximal values of V p and S BET. These results can be explained by burn-off mainly of the outer layers of carbon particles and a small degree of burn-off in pores. The second process is maximal for L1000 as the most porous sample studied. An increase in the activation temperature leads to an increase in the conductivity of carbons that is maximal for L1000. This can be explained by deeper activation of this carbon and more effective removal of the O- and H-containing functionalities.



2D-nonlocal density functional theory


Activated carbon




Differential thermal analysis


Differential thermogravimetry




Pore size distribution


Quenched solid density functional theory


Self-consistent regularization


Transmission electron microscopy




Temperature-programmed desorption mass-spectroscopy


X-ray diffraction



This work was supported by the Ministry of Education and Science of Ukraine (project no. 0113U001504c).

Authors’ Contributions

IFM performed the problem definition, analyzed the IR-spectra and TEM images, and participated in the discussion of the experimental results. VIM stated the choice method and subjects of investigation; performed the XRD, low-temperature porometry, and impedance spectroscopy experiments; and participated in the analysis and interpretation of the data. VMS fabricated the initial standards and performed TG/DTG/DTA the experiment. VMG calculated the porous structure parameters of explored standards, analyzed the XRD and TPDMS spectra, participated in the analysis and interpretation of data, and wrote the paper. All authors read and approved the final version.

Authors’ Information

IFM is the Head of the Organic and Analytical Chemistry Department and a senior researcher at Vasyl Stefanyk PreCarpathian National University, Ivano-Frankivsk, Ukraine. VIM is an associate professor at the Physics and Technology Department, Vasyl Stefanyk PreCarpathian National University, Ivano-Frankivsk, Ukraine. VMS is a research assistant at the Organic and Analytical Chemistry Department, Vasyl Stefanyk PreCarpathian National University, Ivano-Frankivsk, Ukraine. VMG is a Professor and Head of the Department of Amorphous and Structurally Ordered Oxides, Chuiko Institute of Surface Chemistry, Kyiv, Ukraine.

Competing Interests

The article contains no information which would touch the personal or financial interests of other people and organizations.

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors’ Affiliations

Vasyl Stefanyk Precarpathian National University
Chuiko Institute of Surface Chemistry


  1. Bansal CR, Donnet JB, Stoeckli F (1988) Active carbon. Marcel Dekker, New YorkGoogle Scholar
  2. Smisek M, Cerny S (1970) Active carbon. Elsevier, AmsterdamGoogle Scholar
  3. Xie Z-L, White RJ, Weber J, Taubert A, Titirici MM (2011) Hierarchical porous carbonaceous materials via ionothermal carbonization of carbohydrates. J Mater Chem 21:7434–7442.View ArticleGoogle Scholar
  4. Huang S, Shi J (2014) Monolithic macroporous carbon materials as high-performance and ultralow-cost sorbents for efficiently solving organic pollution. Ind Eng Chem Res 53:4888–4893View ArticleGoogle Scholar
  5. Nowicki P, Skrzypczak M, Pietrzak R (2010) Effect of activation method on the physicochemical properties and NO2 removal abilities of sorbents obtained from plum stones (Prunus domestica). Chem Eng J 162:723–729View ArticleGoogle Scholar
  6. Yagmur E, Ozmak M, Actas Z (2008) A novel method for production of activated carbon from waster tea by chemical activation with microwave energy. Fuel 87:3278–3285View ArticleGoogle Scholar
  7. Lv Y, Gan L, Liu M, Xiong W, Xu Z, Zhu D, Wright DS (2012) A self-template synthesis of hierarchical porous carbon foams based on banana peel for supercapacitor electrodes. J Power Sources 209:152–157View ArticleGoogle Scholar
  8. Lee J, Yoon S, Hyeon T, Oh SM, Kim KB (1999) Synthesis of a new mesoporous carbon and its application to electrochemical double-layer capacitors. Chem Commun 21:2177–2178View ArticleGoogle Scholar
  9. Byrne CE, Nagle DC (1997) Carbonization of wood for advanced materials applications. Carbon 35:259–266View ArticleGoogle Scholar
  10. Falco C, Marco-Lozar JP, Salinas-Torres D, Morallón E, Cazorla-Amorós D, Titirici MM, Lozano-Castelló D (2013) Tailoring the porosity of chemically activated hydrothermal carbons: influence of the precursor and hydrothermal carbonization temperature. Carbon 62:346–355View ArticleGoogle Scholar
  11. Fuertes AB, Sevilla M (2015) High-surface area carbons from renewable sources with a bimodal micro-mesoporosity for high-performance ionic liquid-based supercapacitors. Carbon 94:41–52View ArticleGoogle Scholar
  12. McEnaney B (2002) Carbonization and graphitization. Phys Technol 5:5–7View ArticleGoogle Scholar
  13. Marsh H, Rodríguez-Reinoso F (2006) Activated carbon. Elsevier, LondonGoogle Scholar
  14. Yu JS, Yoon SB, Chai GS (2001) Ordered uniform porous carbon by carbonization of sugars. Carbon 39:1442–1446View ArticleGoogle Scholar
  15. Lee JW, Kwon TO, Moon IS (2004) Adsorption of monosaccharides, disaccharides, and maltooligosaccharides on activated carbon for separation of maltopentaose. Carbon 42:371–380View ArticleGoogle Scholar
  16. Sevilla M, Sanchís C, Valdés-Solís T, Morallón E, Fuertes AB (2008) Direct synthesis of graphitic carbon nanostructures from saccharides and their use as electrocatalytic supports. Carbon 46:931–939View ArticleGoogle Scholar
  17. Ryu J, Suh YW, Suh DJ, Ahn DJ (2010) Hydrothermal preparation of carbon microspheres from mono-saccharides and phenolic compounds. Carbon 48:1990–1998View ArticleGoogle Scholar
  18. Lee JS, Mayes RT, Luo H, Dai S (2010) Ionothermal carbonization of sugars in a protic ionic liquid under ambient conditions. Carbon 48:3364–3368View ArticleGoogle Scholar
  19. St. Dennis JE, Venkataraman P, He J, John VT, Obrey SJ, Currier RP, Lebrón-Colón M, Sola FJ, Meador MA (2011) Rod-like carbon nanostructures produced by the direct pyrolysis of α-cyclodextrin. Carbon 49:718–722View ArticleGoogle Scholar
  20. Narasimman R, Prabhakaran K (2012) Preparation of low density carbon foams by foaming molten sucrose using an aluminium nitrate blowing agent. Carbon 50:1999–2009View ArticleGoogle Scholar
  21. Narasimman R, Prabhakaran K (2012) Preparation of carbon foams by thermo-foaming of activated carbon powder dispersions in an aqueous sucrose resin. Carbon 50:5583–5593View ArticleGoogle Scholar
  22. Kalijadis A, Đorđević J, Trtić-Petrović T, Vukčević M, Popović M, Maksimović V, Rakočević Z, Laušević Z (2015) Preparation of boron-doped hydrothermal carbon from glucose for carbon paste electrode. Carbon 95:42–50View ArticleGoogle Scholar
  23. Romero-Anaya AJ, Ouzzine M, Lillo-Ródenas MA, Linares-Solano A (2014) Spherical carbons: synthesis, characterization and activation processes. Carbon 68:296–307View ArticleGoogle Scholar
  24. Rouzaud JN, Oberlin A (1989) Structure, microtexture, and optical properties of anthracene and saccharose-based carbons. Carbon 27:517–529View ArticleGoogle Scholar
  25. Shuttleworth PS, Budarin VL, White RJ, Gun’ko VM, Luque R, Clark JH (2013) Molecular-level understanding of the carbonisation of polysaccharides. Chem Eur J 19:9351–9357View ArticleGoogle Scholar
  26. Tennison SR (1998) Phenolic resin derived activated carbons. Appl Cat A Gen 173:289–311View ArticleGoogle Scholar
  27. Gun’ko VM, Kozynchenko OP, Turov VV, Tennison SR, Zarko VI, Nychiporuk YM, Kulik TV, Palyanytsya BB, Osovskii VD, Ptushinskii YG, Turov AV (2008) Structural and adsorption studies of activated carbons derived from porous phenolic resins. Colloids Surf A: Physicochem Eng Aspects 317:377–387View ArticleGoogle Scholar
  28. Gun’ko VM, Turov VV, Kozynchenko OP, Palijczuk D, Szmigielski R, Kerus SV, Borysenko MV, Pakhlov EM, Gorbik PP (2008) Characteristics of adsorption phase with water/organic mixtures at a surface of activated carbons possessing intraparticle and textural porosities. Appl Surf Sci 254:3220–3231View ArticleGoogle Scholar
  29. Lillo-Ródenas MA, Cazorla-Amorós D, Linares-Solano A (2003) Understanding chemical reactions between carbons and NaOH and KOH: an insight into the chemical activation mechanism. Carbon 41:267–275View ArticleGoogle Scholar
  30. Carvalho AP, Gomes M, Mestre AS, Pires J, de Carvalho MB (2004) Activated carbons from cork waste by chemical activation with K2CO3: application to adsorption of natural gas components. Carbon 42:672–674View ArticleGoogle Scholar
  31. Wang H, Zhong Y, Li Q, Yang J, Dai Q (2008) Cationic starch as a precursor to prepare porous activated carbon for application in supercapacitor electrodes. J Phys Chem Solids 69:2420–2425View ArticleGoogle Scholar
  32. Rodriguez-Reinoso F, McEnaney B, Rouquerol J, Unger K (eds) (2002) Studies in surface science and catalysis. Vol. 144. Characterisation of porous solids VI. Elsevier Science, AmsterdamGoogle Scholar
  33. Armandi M, Bonelli B, Geobaldo F, Garrone E (2010) Nanoporous carbon materials obtained by sucrose carbonization in the presence of KOH. Micropor Mesopor Mater 132:414–420View ArticleGoogle Scholar
  34. Shcherban ND, Ilyin VG (2015) Matrix and bulk synthesis, activation and functionalization of nanoporous carbon adsorbents. Chem Phys Technol Surf 6:97–121Google Scholar
  35. Garrett RH, Grisham CM (2005) Biochemistry, 3rd edn. Thomson Brooks/Cole, BelmontGoogle Scholar
  36. Bochkov AF, Afanasyev VA, Zaikov GE (1980) Carbohydrates. Nauka, MoscowGoogle Scholar
  37. Anslyn EV, Dougherty DA (2006) Modern physical organic chemistry. University Science, SausalitoGoogle Scholar
  38. Gun’ko VM, Leboda R (2002) Carbon-silica gel adsorbents. In: Hubbard AT (ed) Encyclopedia of surface and colloid science. Marcel Dekker, New York, pp 864–878Google Scholar
  39. Skubiszewska-Zięba J, Leboda R, Seledets O, Gun’ko VM (2003) Effect of preparation conditions of carbon-silica adsorbents based on mesoporous silica gel Si-100 and carbonised glucose on their pore structure. Colloids Surf A: Physicochem Eng Aspects 231:39–49View ArticleGoogle Scholar
  40. Gor GY, Thommes M, Cychosz KA, Neimark AV (2012) Quenched solid density functional theory method for characterization of mesoporous carbons by nitrogen adsorption. Carbon 50:1583–1590.View ArticleGoogle Scholar
  41. Jagiello J, Olivier JP (2013) 2D-NLDFT adsorption models for carbon slit-shaped pores with surface energetical heterogeneity and geometrical corrugation. Carbon 55:70–80View ArticleGoogle Scholar
  42. Jagiello J, Ania CO, Parra JB, Cook C (2015) Dual gas analysis of microporous carbons using 2D-NLDFT heterogeneous surface model and combined adsorption data of N2 and CO2. Carbon 91:330–337View ArticleGoogle Scholar
  43. Gun’ko VM (2014) Composite materials: textural characteristics. Applied Surface Sci 307:444–454View ArticleGoogle Scholar
  44. Fiji. Accessed Aug 2015
  45. Gun’ko VM, Kozynchenko OP, Tennison SR, Leboda R, Skubiszewska-Zieba J, Mikhalovsky SV (2012) Comparative study of nanopores in activated carbons by HRTEM and adsorption methods. Carbon 50:3146–3153Google Scholar
  46. Prodanov D. Accessed Aug 2015
  47. Pokrovsky VA, Chuiko AA (2001) Temperature-programmed desorption mass spectrometry and features non-isometric reactions on the surface of dispersed solids. In: Chuiko AA (ed) The chemistry of silica surface, vol 1, UkrINTEI, Kiev, Part., pp 79–116Google Scholar
  48. Kulyk TV, Palyanytsya BB, Galagan NP (2003) Molecular self-organization in nanosized particles-carbohydrates systems. Nanosystems Nanomaterials Nanotechnologies 1:681–690Google Scholar
  49. Abdullah MH, Yusoff AN (1996) Complex impedance and dielectric properties of an Mg-Zn ferrite. J Alloy Comp 233:129–135View ArticleGoogle Scholar
  50. Gregg SJ, Sing KSW (1982) Adsorption, surface area and porosity, 2nd edn. Academic, LondonGoogle Scholar
  51. Ostafiychuk BK, Mandzyuk VI, Kulyk YO, Nagirna NI (2014) SAXS investigation of nanoporous structure of thermal-modified carbon material. Nanoscale Res Lett 9:1–6View ArticleGoogle Scholar
  52. Russo C, Stanzione F, Tregrossi A, Ciajolo A (2014) Infrared spectroscopy of some carbon-based materials relevant in combustion: qualitative and quantitative analysis of hydrogen. Carbon 74:127–138View ArticleGoogle Scholar
  53. Zawadzki J (1988) Infrared spectroscopy in surface chemistry of carbons. In: Thrower PA (ed) Chemistry and physics of carbon, vol 21. Dekker, New York, pp 147–380Google Scholar
  54. Bellamy LJ (1975) The infra-red spectra of complex molecules, 3rd edn. Chapman and Hall, LondonView ArticleGoogle Scholar
  55. Gómez-Serrano V, Piriz-Almeida FN, Durán-Valle CJ, Pastor-Villegas J (1999) Formation of oxygen structures by air activation. A study by FT-IR spectroscopy. Carbon 37:1517–1528View ArticleGoogle Scholar
  56. Fanning PE, Vannice MA (1993) A DRIFTS study of the formation of surface groups on carbon by oxidation. Carbon 31:721–730View ArticleGoogle Scholar
  57. Biniak S, Swiatkowski A, Pakula M (2001) Electrochemical studies of phenomena at active carbon-electrolyte solution interfaces. In: Radovic LR (ed) Chemistry and physics of carbon, vol 27. Marcel Dekker Inc, New York, pp 125–225Google Scholar


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