The non-isothermal decomposition kinetics of glycine was investigated using analyzer DTG-60. TG experiments were carried out under dynamic nitrogen atmosphere of 30 mL min−1 with heating rates of 10, 14, 18 and 22 K min−1. The kinetic parameters such as activation energy (E), exponential factor (A) and reaction order (n) were evaluated by Flynn–Wall–Ozawa, Doyle, Kissinger and Šatava-Šesták methods. The results show that the non-isothermal decomposition mechanism of glycine corresponds to nucleation and growth, following the Avrami–Erofeev equation with n = 1/3. Moreover, thermodynamic properties of the non-isothermal decomposition process such as the change in the values of enthalpy (ΔH), entropy (ΔS) and Gibbs free energy (ΔG) were calculated.Highlights► Thermal decomposition kinetic of the glycine was studied by TG-DTA methods. ► F–W–O, Doyle, Kissinger and Šatava-Šesták methods were applied. ► The thermal decomposition mechanism of glycine are nucleation and growth. ► The thermodynamic parameters of decomposition of glycine has been confirmed.

Using a laser monitoring technique, the solubility data of taurine in water and aqueous solutions of methanol, ethanol, and 2-propanol were measured over the temperature range from (274.05 to 353.05) K. From the experimental data, the solubility data of taurine in the mixtures of water + methanol, water + ethanol, and water + 2-propanol were found to increase with increasing temperature and decrease with increasing concentration of methanol, ethanol, and 2-propanol in aqueous solution. Also, the water + ethanol solution was a better solvent for the purification of taurine. The Apelblat equation, the simplified model of ideal solution, and the λh equation were used to correlate the solubility data; the results showed that the three models mentioned above agreed well with the experimental data, and the Apelblat equation was the most accurate of all of these for these systems.

The solubilities of imidacloprid in water, methanol, ethanol, acetone, 2-butanone, dichloromethane, 1,2-dichloroethane, and trichloromethane were measured at temperatures from (293.15 to 353.15) K by a synthetic method at atmospheric pressure. The solubilities were correlated by the λh model, in which new parameters were introduced to express the activity coefficients of imidacloprid, determined from the experimental data. The experimental data were also correlated with the Apelblat equation.

The molar heat capacities (Cp) of guaiacol (CAS 90-50-1) and acetyl guaiacol ester (AGE, CAS 613-70-7) were determinated from 290 K to 350 K by differential scanning calorimetry (DSC), and expressed as a function of temperature. Two kinds of group contribution models were used to estimate the molar heat capacities of both guaiacol and AGE, the average relative deviation is less than 10%. The standard molar enthalpies of combustion of guaiacol and AGE were − 3590.0 kJ·mol− 1 and − 4522.1 kJ·mol− 1 by a precise thermal isolation Oxygen Bomb Calorimeter. The standard molar enthalpies of formation of guaiacol and AGE in a liquid state at 298.15 K were calculated to be − 307.95 kJ·mol− 1 and − 448.72 kJ·mol− 1, respectively, based on the standard molar enthalpies of combustion. The thermodynamic properties are useful for exploiting the new synthesis method, engineering design and industry production of AGE using guaiacol as a raw material.

Vapor-liquid equilibrium data (T, x, y) of binary system 1,2-epoxycyclohexane+1,2-dichloroethane were determined experimentally by using a modified ROSE-Williams equilibrium vaporization system at 101.33 kPa. The results show that this binary system does not have azeotropic point. The vapor-liquid equilibrium data are in thermodynamic consistency. The binary interaction parameters in the Wilson equation are presented with the correlation of vapor-liquid equilibrium data. The measurements of liquid phase composition and bubble point temperature are well represented by the Wilson equation. Values of vapor molecular fractions and activity coefficients from the Wilson equation are presented. This work provides important engineering data for the separation of 1,2-dichloroethane and 1,2-epoxycyclohexane .