rgy cycle and use the Standard Enthalpies of combustion values in the table belov e enthalpy of formation of butane, CH10(9). Explain how the value obtained her ent from the value obtained using calorimetry. Substance Enthalpy of Combustion/kJ mol Co H2(g) CAH10(g) -394 -286 -2876 t forms must be available for Open Awards external moderation purposes. Page 6 of 12 he enthalpy change for the dissolution of (NH4)2SO4(s) using the enthalpyc provided below: (remember to write the balanced equation for the dissolutio ng state symbols). Explain how the value obtained here might be different from th using calorimetry. Compound Enthalpies of formation (kJmol") (NH.)2SO4 (0) -1380.9 (NH:)" (ac) -143.5 1009 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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