Problem: 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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We are being asked to determine the expected enthalpy of CS2 relative to CO2


Enthalpy of evaporation is related to boiling point. 

  • enthalpy of vaporization increases as boiling point increase


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)


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Problem Details

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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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.