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.
FREE Expert Solution
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)
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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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Intermolecular Forces and Physical Properties concept. If you need more Intermolecular Forces and Physical Properties practice, you can also practice Intermolecular Forces and Physical Properties practice problems.
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Based on our data, we think this problem is relevant for Professor Wasalathanthri's class at UCONN.
What textbook is this problem found in?
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.