Final answer:
Particle size and intermolecular forces are the two factors of real gases that impact the Ideal Gas Law, as they cause deviations from the assumptions of ideal gases which have no volume and no attractive forces.
Step-by-step explanation:
The two factors of 'real gases' that can have an effect on the Ideal Gas Law are particle size and intermolecular forces. This diverges from the ideal gas assumptions which treat gases as point particles with no volume and no attractive forces between them. In real gases, the finite volume of particles affects the calculations of pressure and volume according to the ideal gas law, hence, adjustments like the van der Waals equation are made to account for the particle size. Likewise, the presence of intermolecular forces can cause gas behavior to vary from predictions of the ideal gas law, especially at high pressures where the attractive forces cause the gas particles to not collide as perfectly elastically as presumed in the kinetic-molecular theory.