What is the total amount of heat required to convert 35.0 g of ice at -22.9 ºC to water at 40.0 ºC? Assume a constant pressure of 1.00 atm. The specific heat of H2O (s) is 2.09 J/g ºC, the specific heat of H2O (l) is 4.18 J/g ºC, and the specific heat of H2O (g) is 1.89 J/g ºC. The heat of fusion is ΔH°fus = 6.01 kJ/mol and the heat of vaporization of water is ΔHºvap = 40.7 kJ/mol. The melting point of water is 0.0º C the boiling point is 100.0 ºC. Remember: q = mCΔT 7.54 x 103 kJ 11.7 kJ 2.50 x 103 kJ 19.2 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.
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What is the total amount of heat required to convert 35.0 g of ice at -22.9 ºC to water at 40.0 ºC? Assume a constant pressure of 1.00 atm. The specific heat of H2O (s) is 2.09 J/g ºC, the specific heat of H2O (l) is 4.18 J/g ºC, and the specific heat of H2O (g) is 1.89 J/g ºC. The heat of fusion is ΔH°fus = 6.01 kJ/mol and the heat of vaporization of water is ΔHºvap = 40.7 kJ/mol. The melting point of water is 0.0º C the boiling point is 100.0 ºC.
Remember: q = mCΔT
7.54 x 103 kJ
11.7 kJ
2.50 x 103 kJ
19.2 kJ
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