Thermal Behavior of Zn（Thr）SO4·H2O

Solid complex Zn(Thr)SO 4·H 2O was prepared in a water acetone system. Under linearly increasing temperature, the non isothermal kinetics and the decomposition mechanism of Zn(Thr)SO 4·H 2O were studied by means of thermogravimetry and IR spectrometry. The thermal decomposition processes of the complex could be divided into three stages. The non isothermal decomposition mechanism and the kinetics parameters of the ligand lost process were obtained from an analysis to the TG DTG curves at various heating rates of 5 0, 10 0, 15 0 and 20 0 K/min by two integral and three differential methods. The results show that the random nucleation and the subsequent growth mechanism ( n =3/2) controlled the ligand lost process, the corresponding activation energy E and pre exponential constant A are 139 96 kJ/mol and 10 11 32 s -1 , respectively. The empirical kinetics model equation was constructed.