3F.19 (b)

[106046096]

Hi! Question 3F.19 (b) asks to explain the following observation in terms of the type and strength of intermolecular forces: The vapor pressure of diethyl ether (C2H5OC2H5) is greater than that of water. Is it due to fewer hydrogen-bonde atoms in diethyl ether than water? Can someone explain this to me, please.

[Laila Alkhouri 3H]

Diethyl ether lacks hydrogen bonding and primarily exhibits van der Waals forces between its molecules. These forces are relatively weaker compared to hydrogen bonding. Water has a strong tendency for hydrogen bonding because it is polar. Hydrogen bonding is a strong intermolecular force that requires a significant amount of energy to break the bonds between water molecules, thus reducing its vapor pressure. Whereas diethyl ether, with weaker van der Waals forces, requires less energy to transition from the liquid phase to the vapor phase, resulting in a higher vapor pressure compared to water. The higher vapor pressure of diethyl ether compared to water is primarily due to the absence of strong hydrogen bonding in diethyl ether, allowing its molecules to escape more easily into the vapor phase at a given temperature. Hopefully that helps! Basically if you look at the forces that each one has it will give you the answer.