Report Table CP.3: Specific Heat of Calculations for the Specific Heat for an Unkhown Metal Mass of unknown metal (g) Mass of calorimeter cup (g) Mass of calorimeter and water (g) Temperature of boiling water bath ("C) Initial temperature of calorimeter water (C) Final temperature of water and metal ("C) Mass of water (g) Temperature change of water (C) (Do not include a negative sign Heat gained by water (cal) (De not include a negative sign) Heat lost by metal (cal) (De net include a negative sign) Temperature change of metal ("C) (Do not include a negative sip Specific heat of metal [cal/g °C) Specific heat of metal [J/(g"C)] O Average specific heat of metal [J/(gc)] ) Identify the Metal based on the average specific heat in J/(g°C) Trial 1 19.947 1.844 47.812 98.900 23.8 24.9 Table view List view ✓ Choose... Lead Copper Iron Trial 2 19.947 1.844 47.030 99.0 22.3 23.4

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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.