Estimate the enthalpy change for the combustion of one mole of acetylene, C2H2, to form carbon dioxide and water vapor. 2C2H2(g) + 5O2(g) ⟶⟶ 4CO2(g) + 2H2O(g) BE(C–H) = 456 kJ/mol BE(C≡C) = 962 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol BE(O–H) = 462 kJ/mol Group of answer choices A.) +653 kJ/mol B.) –1010 kJ/mol C.) –1759 kJ/mol D.) –155 kJ/mol E.) +1010 kJ/mol
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.
Estimate the enthalpy change for the combustion of one mole of acetylene, C2H2, to form carbon dioxide and water vapor.
2C2H2(g) + 5O2(g) ⟶⟶ 4CO2(g) + 2H2O(g)
BE(C–H) = 456 kJ/mol
BE(C≡C) = 962 kJ/mol
BE(O=O) = 499 kJ/mol
BE(C=O) = 802 kJ/mol
BE(O–H) = 462 kJ/mol
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