Gas Stoichiometry question?

"Under high pressure and low temperature", a real gas deviates most from ideal behavior.

Explanation :

Two assumptions of ideal gas :
(1) The size of the gaseous molecules is negligible when compared with the intermolecular distances.
(2) There is no interaction between gaseous molecules.

Under high pressure and low temperature, the gaseous molecules are close together. Therefore :
▪ The size of the gaseous molecules is significant when compared with the short intermolecular distances. Assumption (1) is not followed.
▪ Van der Waals' forces exist between the close gaseous molecules.