Part I Consider the following CHEMICAL CHANGE: Acetylene (C₂H₂) combusts in oxygen to form carbon dioxide and water. Estimate the enthalpy of combustion of acetylene using bond energies data. Calculate the enthalpy of combustion of one mole of C₂H₂ using heats of formation data found on the course website using your personal wireless device. Single Bond Energies (kJ/mol of bonds) H C N 0 S F Cl H 436 C N 413 346 391 305 163 463 358 201 146 347 272 226 565 485 283 190 284 155 O S F Cl 432 339 192 218 255 253 242 Multiple Bond Energies (kJ/mol of bonds) C-C 602 C-N 615 C=0 799 C=C 835 N=N 418 C=N 887 0=0 498 C=0 1072 N N 945
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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