Assertion : Molar enthalpy of vaporisation of water is different from ethanol.
Reason : Water is more polar than ethanol.

$H_2O$ is a liquid while $H_2S$ is a gas due to:

Which of the following hydrogen bonds is the strongest?

In which of the following is the strongest hydrogen bonding observed?

Use the information and data given below to answer the questions $(a)$ to $(c)$. Stronger intermolecular forces result in higher boiling point.
Strength of London forces increases with the number of electrons in the molecule.
Boiling points of $HF, HCl, HBr$ and $HI$ are $293 \ K, 189 \ K, 200 \ K$ and $238 \ K$ respectively.
$(a)$ Which type of intermolecular forces are present in the molecules $HF, HCl, HBr$ and $HI$?
$(b)$ Looking at the trend of boiling points of $HCl, HBr$ and $HI$,explain out of dipole-dipole interaction and London interaction,which one is predominant here.
$(c)$ Why is the boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest?

The vapour pressure of $o-$nitrophenol at any given temperature is predicted to be