Problem: Dichloromethane has a greater solubility in water than in carbon tetrachloride and the two have significantly different vapor pressures at 20°C. See the table below.Explain the solubility difference between the two compounds in terms of the intermolecular forces present in both molecules.In terms of the intermolecular forces, explain the difference in vapor pressure between the two compounds.

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We are being asked to explain the difference in vapor pressure between dichloromethane and carbon tetrachloride.


Vapor pressure

▪ is the pressure exerted by a vapor in equilibrium with its condensed phase
▪ highly influenced by intermolecular forces between molecules


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

Dichloromethane has a greater solubility in water than in carbon tetrachloride and the two have significantly different vapor pressures at 20°C. See the table below.

Explain the solubility difference between the two compounds in terms of the intermolecular forces present in both molecules.

In terms of the intermolecular forces, explain the difference in vapor pressure between the two compounds.

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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.