To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 12.0 g, and its initial temperature is -14.0 °C. The water resulting from the melted ice reaches the temperature of his skin, 29.1 °C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table. q= Quantity Enthalpy of fusion at 0°C Enthalpy of vaporization at 100°C Specific heat of solid H₂O (ice) Specific heat of liquid H₂O (water) Specific heat of gaseous H₂O (steam) per gram 333.6 J/g 2257 J/g 2.087 J/(g.°C) * 4.184 J/(g.°C) * 2.000 J/(g.°C) * per mole 6010. J/mol 40660 J/mol 37.60 J/(mol.°C) * 75.37 J/(mol.°C) * 36.03 J/(mol.°C) *
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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