Geopolymers
Inorganic polymeric new materials
Author:
Author:
Edwin H. Battley
Edwin H. Battley
Department of Ecology and Evolution, Stony Brook University, Stony Brook, NY, 11794–5245, USA
64 Cedar Street, Stony Brook, NY, 11790, USA
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64 Cedar Street, Stony Brook, NY, 11790, USA
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Abstract
The equation ΔrX = ΔrH − ΔrQ represents a calculated free-energy change when the exchange of absorbed thermal energy in a chemical system represented by TΔrS in the Gibbs free-energy equation is replaced by ΔrQ. The symbol Q is used in place of H [enthalpy = HT − H0 = HT] to represent absorbed thermal energy. Acquiring the experimental data for determining both S and Q requires the use of a low-temperature calorimeter to measure Cp as a function of T/K and these are not generally available. In a previous study it was demonstrated that for one unit-carbon formula dry weight of cells, ΔfSbiomass = − 0.813 ∑Satoms and Sbiomass = 0.187 ∑Satoms, where ∑Satoms represents the sum of the entropies of the numbers and kinds of atoms in the biomass. Using similar techniques, it is shown here that ΔfQbiomass = − 0.648 ∑Qatoms and that Qbiomass = 0.352 ∑Qatoms, where ∑Qatoms represents the sum of the absorbed thermal energies of the numbers and kinds of atoms in the biomass. Because mathematically the value of TS for solid substances is twice that of Q for the same T/K (usually referenced at 298.15 K), one of these values must be physically incorrect. There cannot be two different values for the quantity of thermal energy which must be absorbed to raise the temperature of the same quantity of the same substance from 0 K to a given temperature. The argument is made that the use of Q is preferable to the use of S in the calculation of free-energy changes.
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1. Battley EH . The thermodynamics of cellular growth. In: Gallagher PK, series editor Handbook of thermal analysis and calorimetry, vol 4, From macromolecules to man (volume editor Kemp RB) Chapter 5. Amsterdam: Elsevier; 1999. p. 219–266 (Table 2, p. 236).
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2. Battley, EH. Growth-reaction equations for Saccharomyces cerevisiae 1960. Physiol Plant 13:192–203 .
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3. Battley, EH Energetics of microbial growth 1987 Wiley New York 450.
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4. Battley, EH. The thermodynamics of growth of Escherichia coli K-12 on succinic acid. Pure Appl Chem. 1993;65:1881–1886 .
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5. Battley, EH. A reevaluation of the thermodynamics of growth of Saccharomyces cerevisiae on glucose, ethanol, and acetic acid. Can J Microbiol. 1995;41:388–398 .
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6. Battley, EH. On the thermodynamics of growth of Pseudomonas saccharophila 1996. Can J Microbiol 42:38–45 .
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7. Wagman DD , Evans WH, Parker VB, Schuum RH, Halow I, Bailey SM, Churney KL, Nuttall RL. The NBS tables of chemical thermodynamic properties. Selected values for inorganic and C1 and C2 organic substances in SI units. J Phys Chem Ref Data. 1982; 11 (2): 7a = (2–10). 7b = (2–11).
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8. Battley, EH, Putnam, RI, Boerio-Goates, J. Heat capacity measurements from 10 K to 300 K and derived thermodynamic functions of lyophilized cells of Saccharomyces cerevisiae including the absolute entropy and the entropy of formation at 298.15 K. Thermochim Acta 1997 298:37–46 .
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10. Morrison, P. A thermodynamic characterization of self-reproduction. Rev Mod Phys. 1964;36:517–524 (Copyright 1964 by the American Physical Society).
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11. Battley, EH, Stone, JR. On the inequality of Qo and TΔSo with respect to solid state organic substances of biological importance. Thermochim Acta 2000 360:1–9 .
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12. Battley, EH. A theoretical approach to the study of the thermodynamics of growth of Saccharomyces cerevisiae (Hansen). Physiol Plant. 1960;13:674–686 .
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13. Battley, EH. On the use of ΔQ 2002 o rather than TΔSo in the calculation of ΔGo accompanying the oxidation or fermentation of catabolic substrates of biological importance in their standard states. Thermochim Acta 394:313–327 (Invert the data in column 4 of Table 7).
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15. Battley, EH. An empirical method for estimating the entropy of formation and the absolute entropy of dried microbial biomass for use in studies on the thermodynamics of microbial growth. Thermochim Acta. 1999;326:7–15 .
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27. Hutchens, JO, Cole, AG, Stout, JW. Heat capacities from 11 to 305 K, entropy, enthalpy, and free energy of formation of serine. J Biol Chem 1963 239:4194–4195.
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29. Putnam, RL, Boerio-Goates, J. Heat capacity measurements and thermodynamic functions of crystalline sucrose at temperatures from 5 K to 342 K. Revised values for Δf G (sucrose, cr, 298.15 K), Δf G (sucrose, aq, 298.15 K), S (sucrose, aq, 298.15 K), and Δr G (298.15 K) for the hydrolysis of aqueous sucrose. J Chem Thermodyn 1993 25:607–613 .
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| Journal of Thermal Analysis and Calorimetry | |
|---|---|
| Language | English |
| Size | A4 |
| Year of Foundation |
1969 |
| Volumes per Year |
1 |
| Issues per Year |
24 |
| Founder | Akadémiai Kiadó |
| Founder's Address |
H-1117 Budapest, Hungary 1516 Budapest, PO Box 245. |
| Publisher | Akadémiai Kiadó Springer Nature Switzerland AG |
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| ISSN | 1388-6150 (Print) |
| ISSN | 1588-2926 (Online) |
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