I. AHrxn for the reaction below was determined using bond dissociation energies (BDES) to be -57 kJ. Using the table of BDE below, find the bond energy for H-Br. H H C=C H H + HBr Bond BDE (kJ/mol) H Br H-C-C-H HH C-C 348 C=C C-H 614 413 C-Br 276 II. Use heats of formation to find the standard heat of reaction (AH° rxn) for the reaction shown above. C₂H4 and HBr are both gases and AH°f for CH3CH₂Br (l) is -85.3 kJ/mol. Use T16-4-1 to find any additional values of AH°f needed. III. Why is there a dfference between the reaction enthalpies calculated by these different approaches?
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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