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Heat Capacities and Nonisothermal Thermal Decomposition Reaction Kinetics of d-Mannitol

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Department of Chemistry, School of Chemical Engineering, Dalian University of Technology, Dalian 116023, China, Material Testing Center, Dalian University of Technology, Dalian 116023, China, and Thermochemistry Laboratory, Dalian Institute of Chemical Physics, Chinese Academy of Sciences, Dalian 116023, China
* Corresponding author. E-mail: [email protected]. Fax: +86-411-84691570. Tel.: +86-411-84379199.
†School of Chemical Engineering, Dalian University of Technology.
‡Material Testing Center, Dalian University of Technology.
§Dalian Institute of Chemical Physics, Chinese Academy of Sciences.
Cite this: J. Chem. Eng. Data 2010, 55, 1, 119–124
Publication Date (Web):July 16, 2009
https://doi.org/10.1021/je900285w
Copyright © 2009 American Chemical Society

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    Abstract

    The low-temperature heat capacity Cp,m of d-mannitol was measured in the temperature range from (80 to 390) K by means of a fully automated adiabatic calorimeter. The dependence of heat capacity on the temperature was fitted to a polynomial equation with the least-squares method. The thermodynamic functions (HTH298.15 K) and (STS298.15 K) were derived from the heat capacity data in the temperature range of (80 to 390) K with an interval of 5 K. The melting temperature, molar enthalpy, and entropy of fusion were determined to be (437.25 ± 0.12) K, (54.69 ± 1.64) kJ·mol−1, and (125.08 ± 3.75) J·K−1·mol−1 by DSC measurements. The thermal stability and nonisothermal thermal decomposition kinetics of the compound were studied by the TG-DTG technique under atmospheric pressure and flowing nitrogen gas conditions. The thermal decomposition process had one mass loss stage, and the apparent activation energy Ea was obtained to be (120.61 ± 1.85) kJ·mol−1 by the Kissinger, Friedman, and Flynn−Wall−Ozawa methods. The Malek method was used to identify the most probable kinetic model SB(m, n). The kinetics model function and the pre-exponential factor A were expressed to be: f(α) = α0.306(1 − α)0.381; ln A = 17.88, respectively.

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