1. Mass of calorimeter 2. Mass of calorimeter + HCI solution 3. Mass of HCI solution 4. Initial temperature of HCI solution 5. Mass of MgO 6. Moles of MgO 7. Final temperature of HCI solution 8. Change in temperature of HCI solution, AT solution 9. Energy released/absorbed by HCI solution, 9solution (Show calculations) 10. Energy released/absorbed by chemical reaction, greaction 11. Enthalpy of chemical reaction in kJ/mole, AH (Show calculations) 12. Average enthalpy of reaction, in kJ/mole. Trial 1 137.97 219.385 74.185 24.0 0.516 0.0128 28.0 4.0 Trial 2 137.97 219.812 74.512 29.0 0.561 0.0139 35.0 6.0
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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