For example, the enthalpy change required to completely vaporize \( 1 \mathrm{~mol} \) liquid water once it has reached the boiling point of \( 100^{\circ} \mathrm{C} \) at 1 bar (the molar enthalpy of vaporization) and the enthalpy change when \( 1 \mathrm{~mol} \) water vapor at \( 100^{\circ} \mathrm{C} \) condenses to liquid water at \( 100^{\circ} \mathrm{C} \) (the molar enthalpy of condensation) have the same values but opposite signs:
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This heat is used to break the intermolecular forces holding the water molecules together in the liquid state, allowing them to move freely in the gas state. This process is endothermic, meaning it absorbs heat, so the enthalpy change (ΔH) is positive. This value Show more…
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