For the complete combustion of 1.000 mole of ethane gas at 298 K and 1 atm pressure, Δ H° = -1560 kJ/mol. What will be the heat released when 8.38 g of ethane is combusted under these conditions?
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.
For the complete combustion of 1.000 mole of ethane gas at 298 K and 1 atm pressure, Δ H° = -1560 kJ/mol. What will be the heat released when 8.38 g of ethane is combusted under these conditions?
The complete combustion reaction for ethane is given as -
C2H6 + 7/2O2 ---> 2CO2 + 3H2O (∆H°=-1560 kJ/mol)
Here , in above Reaction,molar mass of ethane is = 12×2+1×6= 30g/mol
It means, 30 gram of ethane on combustion releases -1560 kJ/mol energy.
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