Magnesium pieces (0.49 g) react in dilute acidic solution (141 mL) as follows: Mg(s) + 2 HCl(aq) →→ MgCl₂(aq) + H₂(g) The temperature of the solution increases from 22.2 °C to 44.8 °C. Determine the enthalpy change for the reaction in kJ per mol Mg(s) that reacts. Magnesiumstukk verdunde suurop volg: (Assume that the specific heat capacity of the solution, and density of HCl(aq) can be approximated by the values for pure water. Furthermore, no heat energy is exchanged with the calorimeter). Die temperatuur van 22.2 °C tot 4- entalpieverander per mol Mg(s) wa (Neem aan dat di hittekapasiteit va digtheid van HCIC deur die waardes gebruik. Verder w met die kalorime
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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