What is the energy of a hydrogen bond?

Which one of the following compounds shows the presence of intramolecular hydrogen bond?

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?

Which of the following interactions lies in the range of $8 - 42 \, kJ/mol$?

The bond angle between $H-O-H$ in ice is closest to

Assertion $(A)$: Hydrogen fluoride has a higher boiling point than other hydrogen halides.
Reason $(R)$: Hydrogen fluoride exhibits strong hydrogen bonding. The correct option among the following is: