art A. Enthalpy Change (HCI - Mg) Mass of magnesium (g) Mass of inner cup and solution (g) Mass of solution (g) nitial temperature of solution (°C) Temperature (°C) after 30 seconds 60 seconds 90 seconds 120 seconds 150 seconds 180 seconds Trial 1 0.369 50.456 21.2 38.4 45.1 45.4 45.4 45.4 45.1 Trial 2 0.395 51.012 21.0 37.8 44.9 45.0 45.5 45.4 45.0 Trial 3 0.341 49.336 22.0 36.6 39.5 44.9 45.0 44.5 43.5 Trial 4 0.345 49.250 22.0 36.7 45.5 45.5 45.5 44.8 44.7 Heat capacity of calorimeter (J/oC) Specific heat of solution (J/goC) 2.1 4.17
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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