Explain why each molecule has a higher vapor pressure at a given temperature than the other in the pair. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer 1. The main reason why CHOH has a higher vapor pressure at a given temperature when compared to CH3 CH2 CH2 OH is that CH3OH
2. The main reasons why CH4 has a higher vapor pressure at a given temperature when compared to CH3 Cl is that CH4and
3. The main reasons why H2CO has a higher vapor pressure at a given temperature when compared to CH3 OH is that H2 COand
does not exhibit dispersion forces
does not exhibit dipole-dipole forces
does not exhibit hydrogen bonding
is polar
has a smaller molar mass

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

dynamic equilibrium is the answer.

thats how its supposed to be