The melting and boiling points of noble gases are very low in comparison to those of other substances of comparable atomic and molecular masses.
This indicates that only weak van der Waal's forces or weak London dispersion forces are present between the atoms of the noble gases in the liquid or the solid state.
The van der Waal's force increases with the increase in the size of the atom, and therefore, in general, the boiling and melting points increase from He to Rn.
Helium boils at 2690C.
Argon has larger mass than helium and have larger dispersion forces. Because of larger size the outer electrons are less tightly held in the larger atoms so that instantaneous dipoles are more easily induced
resulting in greater interaction between argon atoms. Therefore, its boiling point (1860C) is more than that of He.
Similarly, because of increased dispersion forces, the boiling and melting points of monoatomic noble gases increase from helium to radon.
So among the given noble gases Xe is having maximum boiling point

The noble gases are a group of elements in the periodic table that are known for their low reactivity and full electron shells. They are characterized by their extremely low boiling points, which increase as you move down the group from helium (He) to xenon (Xe).

The boiling point of a substance is the temperature at which it changes from a liquid to a gas. It is determined by the strength of the intermolecular forces between the particles of the substance. In the case of noble gases, these forces are known as London dispersion forces or van der Waals forces.

Helium, the lightest noble gas, has the lowest boiling point of all the noble gases. It has only two electrons and a very small atomic size, which results in weak intermolecular forces. As a result, helium boils at a temperature of -268.93°C (-452.07°F).

As we move down the group, the atomic size of the noble gases increases, and the number of electrons also increases. This leads to an increase in the strength of the London dispersion forces. The larger the atoms and the more electrons they have, the greater the temporary fluctuations in electron distribution, and the stronger the attractive forces between the atoms.

Xenon, the heaviest noble gas, has the highest boiling point among the noble gases. It has 54 electrons and a larger atomic size compared to the other noble gases. The increased number of electrons and larger atomic size result in stronger intermolecular forces. Xenon boils at a temperature of -108.1°C (-162.5°F), which is significantly higher than the boiling points of helium, neon, and krypton.

In summary, the noble gas with the highest boiling point is xenon (Xe). Its larger atomic size and increased number of electrons lead to stronger intermolecular forces, resulting in a higher boiling point compared to the other noble gases.