Final answer:
The incorrect assumptions made for ideal gases regarding real molecules include the negligible volume of gas particles and the lack of intermolecular forces. These factors cause deviations from ideal behavior, especially under high pressure or low temperature.
Step-by-step explanation:
The assumptions made for ideal gases that are incorrect in real molecules are based on the kinetic molecular theory. This theory assumes that gas particles have no significant volume and do not attract or repel each other. However in real gases, molecules do occupy space and interact with each other through attractive and repulsive forces. Specifically, the incorrect assumptions are:
The negligible volume of gas particles
The lack of intermolecular forces between gas particles
These factors can cause deviations from ideal behavior, particularly under conditions of high pressure or low temperature. At high pressures the volume of gas molecules becomes significant compared to the total volume and intermolecular attractions can affect the gas properties. At low temperatures, gases are more likely to liquefy which is also not predicted by the kinetic molecular theory. Therefore, the assumption that is most incorrect for real molecules is 'c) Random motion and negligible volume of gas particles', as real gas particles have a volume and do exert intermolecular forces.