We are being asked to determine the expected enthalpy of CS2 relative to CO2
Enthalpy of evaporation is related to boiling point.
Boiling Point and Intermolecular Forces
▪stronger IMF → molecules are strongly held together
▪more energy is required to break them apart → higher temperature required
▪ therefore: higher boiling (↑ BP) → stronger IMF (↑ IMF)
The enthalpy of vaporization of CO2(l) is 9.8 kJ/mol. Would you expect the enthalpy of vaporization of CS2(l) to be 28 kJ/mol, 9.8 kJ/mol, or −8.4 kJ/mol? Discuss the plausibility of each of these answers.
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