Calculating the Change in Bond Enthaly: The Difference between Complete and Incomplete Burning
It is crucial to be able to differentiate between complete and incomplete combustion by understanding bond enthalpy. Bond enthalpy is defined as “the amount of energy required to break one mole of bonds of a given kind” (“Bond enthalpy”). The energy that is released during the formation of bonds is called the “change in bond enthalpy”. The change in bond energy for any given reaction is used to understand differences between incomplete and complete combustion. The complete combustion of butanol, CH100 + 602, – 4CO2+ 5H20), releases more energy that the incomplete combustion (CAH100 + 402, – 4CO2+ 5H20). Calculating the changes in bond enthalpy can show this. The energy required to complete butanol combustion is (5×803+5×467) + (2×416+2×356+6×336+2×498) = 9,898 KJ. However, for incomplete butanol combustion, (4×803+5×467) + (2×416+2×356+6×336+2×498) = 8,932kJ. According to Lubin, 2019, the total combustion of butanol is more efficient than incomplete combustion.