The molar enthalpy of vaporization of a liquid at its normal boiling point is 39.16 kJ mol-1. When a liquid boils some part of the enthalpy is used in converting the liquid into vapor. The remaining is used in expansion work of the vapor against the external pressure. Calculate what percentage of the enthalpy of vaporization of this liquid is used for the expansion work. Assume that the vapor behaves ideally and that the molar volume of the liquid can be neglected when compared to the molar volume of the vapor. At the normal boiling point of liquid 466.6K, the pressure is 1.00 atm (exactly) by definition.

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The molar enthalpy of vaporization of a liquid at its normal boiling point is 39.16 kJ mol-1. When a liquid boils some part of the enthalpy is used in converting the liquid into vapor. The remaining is used in expansion work of the vapor against the external pressure. Calculate what percentage of the enthalpy of vaporization of this liquid is used for the expansion work. Assume that the vapor behaves ideally and that the molar volume of the liquid can be neglected when compared to the molar volume of the vapor. At the normal boiling point of liquid 466.6K, the pressure is 1.00 atm (exactly) by definition.

 
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