Problem: Which of the following substances most likely has the largest enthalpy of vaporization? (a) CH4(b) CH3CH3(c) CH3CH2—OH(d) HO-CH2CH2—OH(e) H2O

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We are being asked to determine which among the choices has the largest enthalpy of vaporization

Enthalpy of vaporization

  • the amount of energy (enthalpy) that must be added to a liquid substance, to transform a quantity of that substance into a gas.

In this case, use the concept of intermolecular forces to determine which has the largest enthalpy of vaporization where the stronger the IMF, the higher the enthalpy of vaporization


Recall that Intermolecular Forces (IMF) are the attractive forces between 2 molecules.

Ion-dipole

 strongest IMF
▪ deals with the attraction between an ion and a polar compound.

 Hydrogen Bonding

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Problem Details

Which of the following substances most likely has the largest enthalpy of vaporization? 

(a) CH4

(b) CH3CH3

(c) CH3CH2—OH

(d) HO-CH2CH2—OH

(e) H2O

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