Kilocalorie per mole
In this article, we will explore the impact of Kilocalorie per mole on various aspects of contemporary society. From its influence on popular culture to its relevance in academia, Kilocalorie per mole has generated extensive debate and controversy that deserves to be analyzed in detail. Throughout these pages, we will analyze the different perspectives that exist around Kilocalorie per mole and how it has shaped the current landscape. Likewise, we will examine its historical role and its projection into the future, in order to understand its true scope and meaning in our daily lives.
The kilocalorie per mole is a unit to measure an amount of energy per number of molecules, atoms, or other similar particles. It is defined as one kilocalorie of energy (1000 thermochemical gram calories) per one mole of substance. The unit symbol is written kcal/mol or kcal⋅mol−1. As typically measured, one kcal/mol represents a temperature increase of one degree Celsius in one liter of water (with a mass of 1 kg) resulting from the reaction of one mole of reagents.
In SI units, one kilocalorie per mole is equal to 4.184 kilojoules per mole (kJ/mol), which comes to approximately 6.9477×10−21 joules per molecule, or about 0.043 eV per molecule. At room temperature (25 °C, 77 °F, or 298.15 K), one kilocalorie per mole is approximately equal to 1.688 kT per molecule.
Even though it is not an SI unit, the kilocalorie per mole is still widely used in chemistry[1] and biology[2] for thermodynamical quantities such as thermodynamic free energy, heat of vaporization, heat of fusion and ionization energy. This is due to a variety of factors, including the ease with which it can be calculated based on the units of measure typically employed in quantifying a chemical reaction, especially in aqueous solution. In addition, for many important biological processes, thermodynamic changes are on a convenient order of magnitude when expressed in kcal/mol. For example, for the reaction of glucose with ATP to form glucose-6-phosphate and ADP, the free energy of reaction is −4.0 kcal/mol using the pH = 7 standard state.[2]
References
- ^ Bach, Robert D. (2006). "General and Theoretical Aspects of the Peroxide Group". In Rappoport, Zvi (ed.). The Chemistry of Peroxides, Volume 2. Chichester: Wiley. p. 12. ISBN 9780470862759.
- ^ a b Cooper, G.M. The Cell: A Molecular Approach. Sunderland, Massachusetts: Sinauer Associates. Retrieved 20 July 2022.
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