The standard enthalpy of combustion is the enthalpy change when one mole of a reactant completely burns in oxygen under standard thermodynamic conditions (although experimental values are usually obtained under different conditions and subsequently adjusted). By definition, the combustion reactions are always particularly exothermic and so enthalpies of combustion are always negative, although the values for individual combustions may vary.
The most common way of calculating the enthalpy change of combustion (or formation) is by using a Hess cycle or by using numerical based bond enthalpies. It is commonly denoted as or . When the enthalpy required is not a combustion, it can be denoted as . Enthalpies of combustion are typically measured using bomb calorimetry, and have units of energy (typically kJ); strictly speaking, the enthalpy change per mole of substance combusted is the standard molar enthalpy of combustion (which typically would have units of kJ mol−1).
Other articles related to "standard enthalpy change of combustion, standard enthalpy change of, combustion":
... Methane (CH4) and Methanol (CH3OH), the standard enthalpy change of the alkane would be greater than the alcohol ( Methane = -890.3 kJ mol−1, Methanol = -726.0 kJ mol−1) ... Since the complete combustion of both of these carbon compounds produce carbon dioxide (CO2) and water (H2O), there is more bond-breaking and bond-making when Methane is burnt ...
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