Publications Internationales

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    Application of NaOH-activated peanut shells as a low-cost adsorbent for the removal of cationic dyes
    (Global NEST, 2025) Hamdache, Farida; Halet, Farid; Bekhti, Saida; Chergui, Abdelmalek; Yeddou, Ahmed Réda; Nadjemi, Boubekeur
    The main purpose of this study is to evaluate the possibility of using a lignocellulosic residue, peanut shells after alkaline activation, as a low-cost adsorbent for the removal of methylene blue dye from aqueous solutions. Adsorption experiments were conducted by varying parameters such as the initial pH aqueous solution, contact time, temperature, and initial concentration of adsorbate. Results show that pH has no apparent effect on methylene blue adsorption; more than 95% of methylene blue was removed. The adsorption capacity of methylene blue was slightly improved when the particle size of the adsorbent and the temperature decreased. A temperature uptake from 298 K to 328 K induced a decrease in the percentage of methylene blue removal from 91.36% to 84.31%. The kinetic data obtained at different concentrations were analyzed using pseudo-first-order and pseudo-second-order kinetic models. Also, the modeling of isotherm was considered by applying Langmuir, Freundlich, and Temkin models. Kinetic and equilibrium data were best represented by pseudo-second-order and Langmuir models respectively according to determination coefficient R2 and error function values. The ultimate adsorption capacity reached approximately 100 mg/g. Thermodynamics findings revealed that the adsorption proposed is exothermic and spontaneous process. These results show that peanut shells can be a potential adsorbent for organic dyes removal from aqueous solutions
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    Experimental investigation of activated carbon prepared from apricot stones material (ASM) adsorbent for removal of malachite green (MG) from aqueous solution
    (SAGE Publications, 2020) Abbas, Moussa
    The adsorption of malachite green onto activated carbon prepared from apricot stones material has been investigated at batch conditions. The effects of contact time (0–60min), initial pH (3–11), agitation speed (100–700 r/min), temperature (298–343K), adsorbent dose (1–10 g/L), and malachite green concentration (4.45–17.6mg/L) on the malachite green adsorption by apricot stones material have been studied. Malachite green removal increases over the contact time until equilibrium. The batch adsorption experiments were carried out to optimize the physical parameters on the malachite green removal efficiency. It has been found that 23.80mg/g at 25 C and 88.05mg/g at 70 C were removed. The kinetic parameters, rate constants and equilibrium adsorption capacities, were calculated and discussed for each kinetic model. The adsorption of malachite green onto apricot stones material is well described by the pseudo second-order equation. The experimental isotherm data were analyzed by different models; the adsorption follows the Langmuir model, providing a better fit of the equilibrium data. The thermodynamics parameters such as the negative free energy DG ( 0.191 to 4.447 kJ/mol) and positive enthalpy DH (50.86 kJ/mol) indicated the spontaneous and endothermic nature of the malachite green adsorption with a chemisorption process
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    Kinetic and thermodynamic studies of the ammonium ions adsorption onto natural Algerian bentonite
    (Taylor & Francis, 2016) Angar, Yassmina; Djelali, Nacer-Eddine; Kebbouche-Gana, Salima
    Adsorption processes are the most recommended complementary techniques applied in the wastewater treatment owing to their low economic cost, recyclability, efficiency and low power consumption. Clays known for this treatment are aluminosilicate minerals which contain different exchangeable ions on their surfaces. In the structure of bentonite surface, several cations have the exchange ability such as calcium, sodium, magnesium and potassium. This propriety is responsible for the adsorption of several cationic water pollutants. In this study, natural bentonite particles of 80 μm in diameter were considered and kept stirring at 200 RPM in a contaminated solution with ammonium ions. The effect of contact time and temperature showed that at an optimal temperature of 30°C and during a short stirring time of 50 min, the removal efficiency could reach its maximum of 53.36%. The kinetic study of the ammonium adsorption reaction on natural bentonite allowed concluding that the reaction is obeyed to the first-order model. Determination of various thermodynamic parameters suggests that the reaction is spontaneous and exothermic
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    Removal of brilliant green (BG) by activated carbon derived from medlar nucleus (ACMN) – Kinetic, isotherms and thermodynamic aspects of adsorption
    (SAGE, 2020) Abbas, Moussa
    Experimental investigations were undertaken to adsorb Brilliant Green (BG) a toxic dye from aqueous medium using activated carbon derived from the medlar nucleus (ACMN). The adsorp- tion was used to remove BG using ACMN as bio-adsorbent to replace activated carbon still expensive. The prepared adsorbent was characterized by the BET surface area measurement, FTIR spectroscopy and X-ray diffraction. Various parameters such as the initial dye concentration (110–200 mg/L), adsorbent dose (1–6 mg/L), initial pH (2–9) and temperature (298–318 K) were studied to observe their effects on the BG adsorption. Batch studies were conducted in order to determine the optimal parameters required to reach the adsorption equilibrium. The maximum adsorption capacity of ACMN for the BG adsorption at 298 K was found to be 833.15 mg/g. The adsorption kinetic data were analyzed by using several kinetic models namely the pseudo-first- order, pseudo-second-order, Elovich equation, intraparticules diffusion model. It was established that the adsorption obeys the pseudo-second-order kinetic model. The evaluation of thermo- dynamics parameters such as the free energy D G ( 10.584 to 6.413 kJ/mol), enthalpy D H (36.439 kJ/mol) and the change of entropy (0.1438 kJ/mol K) indicated a spontaneous and endo- thermic nature of the reaction with a chemisorption process. The present adsorbent may be considered as an alternative for the better performance of the BG removal from aqueous medium.
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    Adsorption of the Coomassie Brilliant Blue (BBC) onto apricot stone activated carbon : kinetic and thermodynamic study
    (Elsevier, 2014) Kaddour, Samia; Abbas, Moussa; Aksil, Tounsia; Cherfi, Abdelhamid
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    Potential of sawdust materials for the removal of dyes and heavy metals : examination of isotherms and kinetics
    (Taylor and Francis, 2016) Sahmoune, Mohamed Nasser; Yeddou, Ahmed Reda
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    Kinetic and equilibrium studies of coomassie blue G-250 adsorption on apricot stone activated carbon
    (2015) Abbas, Moussa; Cherfi, Abdelhamid; Kaddour, Samia; Aksil, Tounsia; Trari, Mohamed
    The preparation of Activated Carbon from Apricot Stone (ASAC) with H3PO4 and its ability to remove the Coomassie Blue (CB) used in textile industry from aqueous solutions are reported in this study. The FTIR spectroscopy is used to get information on interactions between the adsorbent and CB. A series of contact time experiments were undertaken in stirred batch adsorber to assess the effect of the system variables. The results were discussed and showed that ASAC can be used in the wastewater treatment. A comparison of two models on the overall adsorption rate showed that the kinetic of adsorption was better described by the pseudo-second order model. The adsorption isotherms of CB onto ASAC are determined and correlated with common isotherms equations. The smaller RMSE values obtained for the Freundlich model indicate the better curve fitting; the monolayer adsorption capacity of CB is found to be 10.09 mg/g at temperature 22.5 °C and 98.022 mg/g at temperature 50 °C and pH ~ 2. The thermodynamic parameters indicate the spontaneous and exothermic nature of the adsorption process. The positive value of the entropy (ΔS) clearly that the randomness in decreased at the solid-solution interface during the CB adsorption onto ASAC, indicating that some structural exchange may occur among the active sites of the adsorbent and the ions. The activation energy (66.161 kJ/ mol) indicates that the chemical adsorption was predominant