Provide an example of the enthalpy of vaporization of different molecules and the strength of their intermolecular forces.

The enthalpy of vaporization varies with the strength of intermolecular forces.

The enthalpy of vaporization is the amount of energy required to vaporize a substance at its boiling point. It is a measure of the strength of intermolecular forces between molecules. The stronger the intermolecular forces, the higher the enthalpy of vaporization.

For example, water has a high enthalpy of vaporization due to its strong hydrogen bonding. The hydrogen bonds between water molecules require a lot of energy to break, which is why water has a high boiling point and a high enthalpy of vaporization.

In contrast, methane has a low enthalpy of vaporization due to its weak London dispersion forces. The London dispersion forces between methane molecules are much weaker than the hydrogen bonds between water molecules, so it takes less energy to vaporize methane.

Another example is ethanol, which has a higher enthalpy of vaporization than methane but lower than water. This is because ethanol has both hydrogen bonding and London dispersion forces, but the hydrogen bonding is not as strong as in water.

Overall, the enthalpy of vaporization is a useful measure of the strength of intermolecular forces between molecules. It can help predict the boiling point and other physical properties of a substance.