Thermochemistry of Heteroatomic Compounds: the Heats of Combustion and Formation of Glycoside and Adenosine Phosphates
Vitaly Ovchinnikov, Ludmila Lapteva
DOI: 10.4236/ijoc.2011.13011   PDF    HTML     4,935 Downloads   10,566 Views   Citations


The heats of combustion of 4th glycoside in the condensed state with the use of the equation ΔcombH=15.7-117.2(N-g) , in which N is a number bond-forming (valence) electrons less the number (g) of lone electron pairs of nitrogen (g = 1) and oxygen (g = 2), have been determined. Such dependence is deduced previously joint for the description of the combustion enthalpies of 17 simple ethers of a cyclic structure and different sugars. The heats of formation ( ΔfHo ) of the mentioned above glycosides were calculated according to the Hess law via two ways: 1) through the use their heats of hydrolysis ( ΔhydrH ), which have been investigated earlier experimentally, 2) with the use the calculated the heats of combustion. The last procedure has been used also for the calculation of the heats of formation of the adenosine tri(ATP)-, di(ADP)- and mono(AMP)phosphates because of such thermochemical parameter is often hard achieved experimentally. The heats of hydrolysis ( ΔfH°hydr ) of ATP into ADP and ADP into AMP were calculated on the basis of their heats of formation in water ( ΔfH°aq ). The free energies of the same process ( ΔhydrG ) were known in literature. Last circumstance give us a possibility to calculate the hydrolysis entropies ( ΔhydrS ) using the Gibbs equation. The entropy values are a large negative, that pointed on the preliminary complex formation between adenosine phosphates and water before the breaking of P-O bonds or P-O-C fragments in its.

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Ovchinnikov, V. and Lapteva, L. (2011) Thermochemistry of Heteroatomic Compounds: the Heats of Combustion and Formation of Glycoside and Adenosine Phosphates. International Journal of Organic Chemistry, 1, 67-70. doi: 10.4236/ijoc.2011.13011.

Conflicts of Interest

The authors declare no conflicts of interest.


[1] D. E. C. Corbribge, “Phosphorus: An Outline of Its Chemistry, Biochemistry, and Technology,” 2nd Edition, Elsevier, Amsterdam-Oxford-New York, 1980.
[2] А. White, Ph. Handler, E. Smith, R. Hill and I. R. Leman, “Principles of Biochemistry,” McGraw-Hill, New York, 1978.
[3] J. A. Gerlt, F. H. Westheimer and J. M. Sturtevant, “The Enthalpies of Hydrolysis of Acyclic, Monocyclic, and Glycoside Cyclic Phosphate Diesters,” The Journal of Biological Chemistry, Vol. 250, 1975, pp. 5059-5067.
[4] J. D. Cox and G. Pilcher, “Thermochemistry of Organic and Organometallic Compounds,” Academic Press, New York, 1970.
[5] V. V. Ovchinnikov and N. R. Muzafarov, “Thermo- Chemistry of Heteroatomic Compounds. Calculation of the Formation Enthalpy for Methyl-α-D-4’,6’-Cyclophos- Phate on the Basis of His Enthalpy of Combustion,” Russian Journal of Organic Chemistry, Vol. 45, No. 1, 2009, pp. 318-319.
[6] S. M. Skuratov, A. A. Strepikheev and M. P. Kozina, “About the Combustion of Five and Six-Membered Het- erocyclic Compounds,” Dokl. Acad. Sci. SSSR, Vol. 117, 1957, pp. 452-454.

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