The combustion of kerosene, represented by the balanced equation 2C12H26(l) + 37O2(g) → 24CO2(g) + 26H2O(g), involves the reaction of hydrocarbons with oxygen to produce carbon dioxide and water, releasing a significant amount of heat in the process.
Given that the enthalpy change for the reaction, ΔHrxn = -1.50 x 104 kJ, indicates the heat released for this specific balanced chemical equation, we can analyze what this means for the combustion of kerosene.
To determine the heat released during the combustion:
- First, recognize the stoichiometry of the reaction: for every 2 moles of C12H26, 1.50 x 104 kJ of energy is released.
- If you know the amount of kerosene you are burning (in moles or mass), you can calculate the total energy released. For example, if you burn 1 mole of kerosene, the energy released would be half of
ΔHrxn, which is-7.5 x 103 kJ.
By understanding the reaction and its enthalpy change, you can effectively use this information for practical applications such as heating with kerosene space heaters or for calculations in chemistry involving energy changes in combustion reactions.