I Review I Constants I Periodic Table Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction: 2H3C – CH3 (g) +702(g)→4CO2(g) + 6H2O(g) Part A Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol. Use average bond energies to calculate AHn for this reaction. TVO AEO ДН-n - kJ
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.
Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction:
2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g)2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g)
Note that the average bond energy for the breaking of a bond in CO2CO2 is 799 kJ/molkJ/mol.
Use average bond energies to calculate ΔHrxnΔHrxn for this reaction.
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