Final answer:
The change of enthalpy for the combustion of one mole of pentane is -3509.6 kJ/mol, indicating that it is an exothermic reaction releasing heat.
Step-by-step explanation:
To calculate the change of enthalpy associated with the combustion of one mole of pentane (C5H12), we will use the concept of standard enthalpy of combustion. This is the amount of heat released when one mole of a substance undergoes complete combustion with oxygen under standard state conditions.
The standard enthalpy of combustion for pentane is typically found in reference literature, as it is an experimentally determined value. For pentane, this value is approximately -3509.6 kJ/mol. Therefore, the enthalpy change for combustion of one mole of pentane is -3509.6 kJ, indicating that the reaction is exothermic, releasing heat into the surroundings.
The calculation could be represented by a balanced chemical equation showing pentane reacting with oxygen to form carbon dioxide and water:
C5H12(l) + 8O2(g) → 5CO2(g) + 6H2O(l)