Adsorption of reactive black 5 (RB5) from aqueous solution onto chitosan was investigated in a batch system. The effects of solution pH, initial dye concentration, and temperature were studied. Adsorption data obtained from different batch experiments were modeled using both pseudo first-and second-order kinetic equations. The equilibrium adsorption data were fitted to the Freundlich, Tempkin, and Langmuir isotherms over a dye concentration range of 45-100 mmol/L. The best results were achieved with the pseudo second-order kinetic and Langmuir isotherm equilibrium models, respectively. The equilibrium adsorption capacity (q e ) was increased with increasing the initial dye concentration and solution temperature, and decreasing solution pH. The chitosan flakes for the adsorption of the dye was regenerated efficiently through the alkaline solution and was then reused for dye removal. The activation energy (E a ) of sorption kinetics was estimated to be 13.88 kJ/mol. Thermodynamic parameters such as changes in free energy (DG), enthalpy (DH), and entropy (DS) were evaluated by applying the van't Hoff equation. The thermodynamics of reactive dye adsorption by chitosan indicates its spontaneous and endothermic nature.

Chitosan was utilized as adsorbent to remove methyl orange (MO) from aqueous solution by adsorption. Batch experiments were conducted to study the effects of pH, initial concentration of adsorbate and temperature on dye adsorption. The kinetic data obtained from different batch experiments were analyzed using both pseudo first-order and pseudo second-order equations. The equilibrium adsorption data were analyzed by using the Freundlich and Langmuir models. The best results were achieved with the pseudo second-order kinetic model and with the Langmuir isotherm equilibrium model. The equilibrium adsorption capacity (qe) increases with increasing the initial concentration of dye and with decreasing pH. The values of qe were found to be slightly increased with increasing solution temperatures. The activation energy (Ea) of sorption kinetics was found to be 10.41 kJ/mol. Thermodynamic parameters such as change in free energy (△G), enthalpy (△H) and entropy (△S) were also discussed

The reactions of active nitrogen with the fluoroethylenes C2H3F, 1,1-C2H2F2, C2HF3, and C2F4 have been investigated in a conventional flow system using a mass spectrometer to detect products and intermediate species. Addition of various gases (H, H2, NH3, CH4, N2O, [Formula: see text], and F) to the reacting mixtures provides evidence that both Hand F atoms play significant roles in the reaction mechanisms, while [Formula: see text] does not. A brief discussion of possible mechanisms is presented.

Absolute rate constants are reported for the reaction of fluorine atoms with nitric oxide in the presence of the third bodies Ar, He, Ne, N2, NO, CO2, CF4, SF6, and C2F6. The values determined in the present study are compared to those found for reactions of Cl, H, and O with NO.

The absolute rate constants for the addition of H atoms to C2H3F, 1,1-C2H2F2, C2HF3, C2H3Cl, 1,1 -C2H2Cl2, C2HCl3, and C2H3Br have been determined at 298 ± 2 K over the pressure range 0.70–1.35 Torr. For each of the compounds, the rate constants are found to undergo a modest increase with pressure. At 1.00 Torr the values determined for the rate constants are: C2H3F, (8.86 ± 1.12) × 10−14; 1,1-C2H2F2, (8.16 ± 0.66) × 10−14; C2HF3, (6.21 ± 0.53) × 10−14; C2H3Cl, (27.0 ± 0.5) × 10−14; 1,1-C2H2Cl2, (59.6 ± 3.4) × 10−14; C2HCl3, (10.4 ± 0.8) × 10−14; C2H3Br, (27.8 ± 2.5) × 10−14; in units of cm3 molecule−1 s−1.