TABLE 9.2 Data Table Mass of Water (mwater) Mass of Metal (mmetal) Boiling Water Temperature (Thigh) Initial Temperature of Water in Calorimeter (Tlow) Final Temperature of Water and Metal in Calorimeter (Teqbm) ATwater = Teqbm - Tlow ATmetal = Teqbm - Thigh Specific Heat of Water (shwater) Heat Transferred to Water (water) Heat Transferred from Metal (metal) Specific Heat of Metal (sh metal) Precision of Your sh metal's Average Specific Heat of Metal Molar Mass of Metal via Dulong and Petit % Error of Your Empirical Molar Mass q=m* SH*AT Trial 1 34.1539 35.312 9 100°C 89.7°C 275°C 185.3°C 175°C 4.184 J/g °C Trial 2 33.9969 35.5919 100°C 96.1°C 278 °C ос 181.9°C 178°C 4.184 J/g °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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