Answer :
Final answer:
The enthalpy change associated with the vaporization of ethanol is 38.6 kJmol−1 at its boiling point of 78 ∘C.
Explanation:
The enthalpy change associated with the vaporization of ethanol is a measure of the amount of heat energy required to convert one mole of ethanol from its liquid state to its gaseous state at a constant temperature and pressure. In the case of ethanol, the enthalpy change is 38.6 kJmol−1 at its boiling point of 78 ∘C.
When a substance vaporizes, it undergoes a phase change from a liquid to a gas. This process requires energy, which is supplied in the form of heat. The enthalpy change of vaporization is a measure of the heat energy absorbed or released during this phase change.
In the case of ethanol, the enthalpy change of vaporization is 38.6 kJmol−1. This means that to convert one mole of ethanol from its liquid state to its gaseous state at 78 ∘C, 38.6 kJ of heat energy is required. This value is specific to ethanol and is a characteristic property of the substance.
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