How much heat energy is required to convert 44.9 g of solid ethanol at -114.5 °C to gasesous ethanol at 160.8 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45J/g °C, and that of gaseous ethanol is 1.43J/g °C. kJ
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.
Given,
44.9 g of solid ethanol at -114°C is converted to gaseous ethanol at 160.8 °C
The molar heat of fusion of ethanol is, ∆H(f) = 4.60 kJ/mol, and its molar heat of vaporization is ∆H(v) = 38.56 kJ/mol.
And also Ethanol has a normal melting point of - 114.5 ° C and a normal boiling point of 78.4°C.
The specific heat capacity of liquid ethanol is S(I) = 2.45 J/g °C, and that of gaseous ethanol is S(g) = 1.43 J/g °C.
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