2 C2H6 (g) + 7 O2 (g) -> 4 CO2 (g) + 6 H2O ∆H° = – 3119 kJ molrxn–1 C2H4 (g) + 3 O2 (g) -> 2 CO2 (g) + 2 H2O ∆H°= – 1411 kJ molrxn–1 2 H2 (g) + O2 (g) -> 2 H2O ∆H° = – 572 kJ molrxn–1 Use the information above to find the ∆H°rxn for the formation of ethene from ethane.
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.
One of the steps in the manufacturing of the plastic polyethylene is to remove H2 from C2H6 (ethane) to produce
C2H4 (ethene), utilizing the reaction below.
C2H6 (g) -> C2H4 (g) + H2 (g) ∆H°rxn = ?
From other experiments conducted, the following thermochemical equations are known.
2 C2H6 (g) + 7 O2 (g) -> 4 CO2 (g) + 6 H2O ∆H° = – 3119 kJ molrxn–1
C2H4 (g) + 3 O2 (g) -> 2 CO2 (g) + 2 H2O ∆H°= – 1411 kJ molrxn–1
2 H2 (g) + O2 (g) -> 2 H2O ∆H° = – 572 kJ molrxn–1
Use the information above to find the ∆H°rxn for the formation of ethene from ethane.
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