**1. Introduction**

838 Thermodynamics – Interaction Studies – Solids, Liquids and Gases

1500K, 3CaO·Al2O3 can not transform to 3CaO·SiO2; but the other calcium aluminates all

4) Reactions among Al2O3, Fe2O3, SiO2 and CaO easily form 2CaO·Al2O3·SiO2 and 4CaO·Al2O3·Fe2O3. 2CaO·Al2O3·SiO2 does not form from the reaction of CaO·Al2O3 and CaO·SiO2, but from the direct reaction among Al2O3, CaO, SiO2. And 4CaO·Al2O3·Fe2O3 is also not formed via mutual reaction of calcium ferrites and sodium aluminates, but from the direct reaction of CaO, Al2O3 and Fe2O3. In thermodynamics, when Al2O3, Fe2O3, SiO2 and CaO coexist, 2CaO·Al2O3·SiO2 and 4CaO·Al2O3·Fe2O3 are firstly formed, and then calcium

Li, B.; Xu, Y. & Choi, J. (1996). Applying Machine Learning Techniques, *Proceedings of ASME* 

Rayi H. S. ; Kundu N.(1986). Thermal analysis studies on the initial stages of iron oxide

Coats A.W. ; Redferm J.P.(1964). Kinetic parameters from thermogravimetric data, *Nature*,

LIU Gui-hua, LI Xiao-bin, PENG Zhi-hong, ZHOU Qiu-sheng(2003). Behavior of calcium silicate in leaching process. *Trans Nonferrous Met Soc China*, January 213−216,2003 Paul S. ; Mukherjee S.(1992). Nonisothermal and isothermal reduction kinetics of iron ore

ZHU Zhongping, JIANG Tao, LI Guanghui, HUANG Zhucheng(2009). Thermodynamics of

ZHOU Qiusheng, QI Tiangui, PENG Zhihong, LIU Guihua, LI Xiaobin(2007).

Barin I., Knacke O.(1997). *Thermochemical properties of inorganic substances*, Berlin:Supplement,

Barin I., Knacke O.(1973). *Thermochemical properties of inorganic substances*, Berlin: Springer,

reaction of alumina during sintering process of high-iron gibbsite-type bauxite, *The* 

Thermodynamics of reaction behavior of ferric oxide during sinter-preparing

agglomerates, *Ironmaking and steelmaking*, March 190~193, 1992

process, *The Chinese Journal of Nonferrous Metals*, Jun 974~978, 2007

*Chinese Journal of Nonferrous Metals*, Dec 2243~2250, 2009

*2010 4th International Conference on Energy Sustainability*, pp.14-17, ISBN 842-6508-

can all react with SiO2 to generate calcium silicates at 800~1700K.

,J

23-3, Phoenix, Arizona, USA, May 17-22, 2010

reduction, *Thermochimi, Acta.* 101:107~118,1986

silicates, calcium aluminates and calcium ferrites.

**5. Symbols used** 

Thermal unit: J

**6. References** 

Thermodynamic temperature: T, K

Amount of substance: mole Standard Gibbs free energy: *GT*

201:68,1964

1997

1973

This chapter is an introduction to the thermodynamics of systems, based on the correlation function formalism, which has been established to determine the thermodynamic properties of simple liquids. The article begins with a preamble describing few general aspects of the liquid state, among others the connection between the phase diagram and the pair potential *u*(*r*), on one hand, and between the structure and the pair correlation function *g*(*r*), on the other hand. The pair correlation function is of major importance in the theory of liquids at equilibrium, because it is required for performing the calculation of the thermodynamic properties of systems modeled by a given pair potential. Then, the article is devoted to the expressions useful for calculating the thermodynamic properties of liquids, in relation with the most relevant features of the potential, and provides a presentation of the perturbation theory developed in the four last decades. The thermodynamic perturbation theory is founded on a judicious separation of the pair potential into two parts. Specifically, one of the greatest successes of the microscopic theory has been the recognition of the quite distinct roles played by the repulsive and attractive parts of the pair potential in predicting many properties of liquids. Much attention has been paid to the hard-sphere potential, which has proved very efficient as natural reference system because it describes fairly well the local order in liquids. As an example, the Yukawa attractive potential is also mentioned.
