Acetylene (C₂H₂) and benzene (C6H6) have the same empirical formula. In fact, benzene can be made from acetylene as follows: 3C₂H₂(g) → CHg (1) kJ The enthalpies of combustion for C₂H₂ and C6H6 are - 1296.6 and-3266.6 respectively. Calculate the standard enthalpies of formation of C₂H₂ and C H. Assume that the products of the combustions are CO₂ (g) and H₂O (1). mol Note: Reference the Thermodynamic properties of pure substances table for additional information. Part: 0/2 Part 1 of 2 Calculate the standard enthalpies of formation of C₂H₂ and C6H6. Be sure your answer has the correct number of significant digits. AH(C₂H₂) = kJ mol Be sure your answer has the correct number of significant digits. AH(CH₂) = kJ mol kJ mol 0.0

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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.