The heat of combustion of glucose, C6H12O6, is 670 kcal/mol. The heat of combustion of ethanol, C2H6O, is 327 kcal/mol. The heat liberated by oxidation of each compound is the same whether is burned in the air or metabolized in the body. On a kcal/g basis, metabolism of which compound liberates more heat?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
The heat of combustion of glucose, C6H12O6, is 670 kcal/mol. The heat of combustion of ethanol, C2H6O, is 327 kcal/mol. The heat liberated by oxidation of each compound is the same whether is burned in the air or metabolized in the body. On a kcal/g basis,
The heat of combustion of glucose, C6H12O6, is = 670 kcal/mol
The heat of combustion of ethanol, C2H6O, is = 327 kcal/mol
We know that the molar mass of glucose is = 180.156 g/mol
The molar mass of ethanol is = 46.07 g/mol
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