Correlation between thermal expansion and heat capacity

Journal Ref.: Computer Coupling of Phase Diagrams and Thermochemistry, CALPHAD, 30 (2006) 354-356

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Abstract

Theoretically predicted linear correlation between the volume coefficient of thermal expansion and the thermal heat capacity was investigated for highly symmetrical atomic arrangements. Normalizing the data of these thermodynamic parameters to the Debye temperature gives practically identical curves from zero Kelvin to the Debye temperature. This result is consistent with the predicted linear correlation. At temperatures higher than the Debye temperature the normalized values of the thermal expansion are always higher than the normalized value of the heat capacity. The detected correlation has significant computational advantage since it allows calculating the volume coefficient of thermal expansion from one experimental data by using the Debye function. Employing the detected linear correlation new description for the volume coefficient of thermal expansion is suggested.

Keywords: Thermal Properties; Thermal expansion; Heat capacity; Correlation; Highly symmetrical atomic arrangements

1. Introduction

The volume coefficient of thermal expansion [α_v] is described as

       (1)

where V is the volume, T is the temperature, and P is the pressure. The volume coefficient of thermal expansion is temperature dependent requiring numerous experiments for its complete description. The experiments are time consuming and technically difficult at extreme temperatures.

The theory of thermal expansion is well defined. The volume expansion can be determined by calculating the anharmonic term of the lattice vibration [ex. 1, 2]. This traditional approach has been challenged by a simple classical model [3, 4] which gave good and excellent agreement with the experimental data of Ne, Ar, Kr, and Xe. In these calculations it was assumed that the potential is Lennard-Jones and that the mean value of the interatomic atomic distance can be used to calculate the thermal expansion.

       (2)

The mean interatomic distance with a good approximation is proportional to the mean vibrational energy per atom in a solid [2]. The thermal energy of a system [Q^thermal] is the product of the mean vibrational energy of an atom and the number of atoms in the system. The zero-term energy of the atoms is not included in the thermal energy. Introducing a constant [a] allows to substitute the mean interatomic distance with the thermal energy of a system. Equation (2) can be rewritten then

       (3)

where n is the number of moles.

The molar thermal heat capacity c(φ) ^thermal is defined as:

       (4)

where φ=g(gas), s(solid), l(liquid). Combining equation (3) and (4) gives

[α_v(T)] _p=0 = a [c(s)^thermal] _p=0       (5)

The molar thermal heat capacity is pressure independent. The pressure has effect on the equilibrium separation [R_o] of the atoms, which is incorporated in the constant. The pressure effect on R_ocan be accommodated by assuming that the introduced constant [a] is pressure dependent.

[α_v(T)] _p = a _p [c(s)^thermal]       (6)

The pressure up to few GPa has minor effect on the heat capacity [5]. In this pressure region the molar thermal heat capacity can be replaced with the constant pressure molar heat capacity.

[α_v(T)] _p = a _p [c(s)] _p       (7)

Equation (7) predicts linear correlation between the volume coefficient of thermal expansion and the molar heat capacity at constant pressure. This correlation will be considered in detail.

2. Correlation between the volume coefficient of thermal expansion and molar heat capacity

Experimental data of highly symmetrical mono-atomic arrangements [6] Ag, Al, Au, Ba, Co, Cr, Cu, Fe, K, Ni, Pb, Pt, Ti, V have been used to investigate the predicted correlation between the volume coefficient of thermal expansion and the molar heat capacity at atmospheric pressure. The experimental values of these two thermodynamic parameters were not necessarily determined at the same temperature. In order to make these parameters comparable, the two data sets were normalized to the Debye temperature. It has been found that the normalized values of the volume coefficient of thermal expansion and the heat capacities are practically identical below the Debye temperature. Above the Debye temperature the normalized values of the volume coefficient of thermal expansion are higher than the normalized values of the heat capacity. The characteristic behavior is shown on Fig. 1. These results are interpreted as follows. The identical curves of the normalized values of the volume coefficient of thermal expansion and molar heat capacity at atmospheric pressure confirm the predicted linear correlation between these thermodynamic parameters from zero Kelvin to the Debye temperature. The higher normalized values of the volume coefficient of thermal expansion above the Debye temperature might be the result of the additional expansion caused by lattice vacancies [7, 8].

3. Computational advantages

Employing the detected linear correlation between the volume coefficient of thermal expansion and the molar thermal heat capacity allows calculating the volume coefficient of thermal expansion from any experiment. Using equation (6) for two different temperatures and dividing equation one by equation two gives

                         (8)

The pressure effect is canceled out in equation (8) by the division. The molar thermal heat capacity can be calculated by using the Debye function [9].

                        (9)

and

                     (10)

where h is the Planck's constant, Ω is the frequency, Ω_Dis the Debye frequency and T_D is the Debye temperature. This equation has to be evaluated numerically [10]. Using the experimental value of the volume coefficient of thermal expansion at the Debye temperature [α(T _D)] the volume coefficient of thermal expansion was calculated between zero Kelvin and the Debye temperature. The calculated and the experimental values are plotted in Fig. 2. Based on visual inspection the correlations are excellent for elements (Ag; Al; Au; Cu; Ni; Pb; Pt) with face centered cubic structure, very good for Co and Ti with hexagonal close packed structure and good for element (Ba; Cr; Fe; K; V) with body centered cubic structure.

4. Temperature independent volume coefficient of thermal expansion

The detected linear correlation between the volume coefficient of thermal expansion and the molar heat capacity at constant pressure allows describing the thermal expansion with a constant coefficient. The volume coefficient of thermal expansion becomes constant if the differential of the temperature is replaced with the differential of the enthalpy (H).

              (11)

Above the Debye temperature the volume coefficient of thermal expansion is not constant. For the investigated solids linear temperature related increase has been detected for the volume coefficient of thermal expansion. This effect can be taken into consideration by the introduction of a new constant [C_α]

       (12)

The temperature independent nature of the new volume coefficient of thermal expansion makes the thermodynamic calculations more convenient. Describing the volume coefficient of thermal expansion by equation (11) instead of equation (1) expresses the physics of the thermal expansion properly since the anharmonic term or the mean atomic distance is proportional to the mean energy per atom and not to the temperature.

5. Conclusions

The theoretically predicted linear correlation between the volume coefficient of thermal expansion and the heat capacity has been confirmed for highly symmetrical mono-atomic arrangements.

The detected correlation allows calculating the volume coefficient of thermal expansion from an experiment conducted at a preferably chosen temperature.

Replacing the differential of the temperature in the derivative of the thermal expansion with the differential of the enthalpy results in a temperature independent volume coefficient of thermal expansion up to the Debye temperature. This new thermodynamic parameter expresses the physical process of the thermal expansion more appropriately and makes the calculations simpler.

References

[1] C. Kittel, Introduction to Solid State Physics 6th edition, New York, Wiley, 1986, p. 114.

[2] R.A. Levy, Principles of Solid State Physics, New York, Academic, 1968, p. 141.

[3] P. Mohazzabi and F. Behroozi, Phys. Rev. B 36 (1987) 9820-9823.

[4] P. Mohazzabi and F. Behroozi, Eur. J. Phys. 18 (1997) 237-240.

[5] J. Garai (2005) physics/0511066

[6] Handbook of Physical Quantities, edited by I. S. Grigoriev and E. Z. Meilikhov, CRC Press, Inc. Boca Raton, FL, USA, 1997.

[7] R.O. Simmons and R.W. Balluffi, Phys. Rev. 117 (1960) 52-61.

[8] Th. Hehenkamp, W. Berger, J.–E. Kluin, Ch. Lüdecke, and J. Wolff, Phys. Rev. B 45 (1992) 1998-2003.

[9] P. Debye, Ann. Physik 39, (1912) 789.

[10] Landolt-Bornstein, Zahlenwerte und Funktionen aus Physic, Chemie, Astronomie, Geophysic, und Technik, II. Band, Eigenschaften der Materie in Ihren Aggregatzustanden, 4 Teil, Kalorische Zustandsgrossen, Springer-Verlag, 1961.

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