Use the molar bond enthalpy data in the table to estimate the value of AHin for the equation rxn CCl4 (g) + 2 F₂ (g) → CF4(g) + 2Cl₂(g) The bonding in the molecules is shown. +++ AH ixn = F-F + CI-CI CI-CI Average molar bond enthalpies (H bond) Bond Bond O-H C=N 0-0 N-H C-O N-N 0=0 N=N C=O N=N C-C F-F C=C Cl-Cl C=C Br-Br C-H H-H C-F H-F C-Cl H-Cl C-Br H-Br C-N H-S C=N S-S kJ.mol-¹ 464 142 351 502 730 347 615 811 414 439 331 276 293 615 kJ.mol-¹ 890 390 159 418 945 155 243 192 435 565 431 368 364 225 kJ.mol-¹
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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