Calculate the number of kilojoules of energy required to convert 30.0 grams of liquid ethanol initially at a temperature of -114.0°C to gas at 150.0°C. kj substance m.p. b.p AHtus AHvap Solid °C °C kJ/mol kJ/mol J/g °C COMUNA 46.069 -114.0 78.0 5.02 0.0 100.0 6.01 78.129 19.0 189.0 74.123 25.2 82.4 Ethanol Water DMSO t-Butanol formula C₂H5OH H₂O C₂H SO C4H₁0O m.w. g/mol 18.015 14.4 6.78 38.6 0.970 40.67 Specific Heat Capacity 48.6 39.1 2.09 1.80 1.97 Liquid J/g °C 2.30 4.184 1.96 2.9 Gas J/g °C 1.94 1.84 1.20 1.73
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.
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