Question

Question #d4d89

Answer 1

`"Hydrogen chloride"` would BEHAVE MUCH LESS ideally than `"helium......"`

Explanation:

Ideality assumes minimal interaction between the gaseous particles. For `"hydrogen chloride"`, a potent intermolecular force can operates: `"hydrogen bonding"`, in that the hydrogen is bound to a strongly electronegative chlorine to give the `""^(-delta)Cl-H^(delta+)` dipole, which can act intermolecularly.

Possibly the best metric with which to compare this is the boiling point of the gases: helium has a normal boiling point of `4*K`; hydrogen chloride boils at `188*K` `-` how is this consistent with the hydrogen bonding argument? Compare also normal the boiling point of `HF`, where hydrogen bonding should be stronger or weaker than in `HCl`?

AS hydrogen chloride also possesses many more electrons than does helium, dispersion forces will also be stronger for `HCl`.