Now, using the table of bond energies, calculate the enthalpy change for... CH3Br + OH --> CH3OH + Br AH = E(Bond energies of the bonds broken) - Σ(Bond energies of the bonds formed What is the AH for this reaction? Write out your work. Average Single Bond Energies (kJ per mole) HCNOF Si P S CI Br I H 436 414 389 464 569 293 318 339 431 368 297 347 293 351 439 289 264 259 330 276 238 159 201 272 209 201 243 138 184 368 351 205 159 540 490 285 255 197 176 213 226 360 289 213 230 331 272 213 213 251 213 TUZ с с N O F Si P S CI Br I LLLL 201 Average Multiple Bond Energies (kJ per mole) N= N 418 N N 946 N=0 590 C N 891 0=0 498 C=C 611 C=C 837 C=0 803 C=0 745 C 0 1075 243 218 209 192 180 151 In CO₂ Only
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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