Step 1: Understand the ideal gas law, which is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.
Step 2: Recognize that the ideal gas law assumes gas particles do not attract or repel each other and that they occupy no volume.
Step 3: Identify the conditions where gas particles are close together, which happens at low temperatures and high pressures.
Step 4: Realize that under these conditions, intermolecular forces (like attraction or repulsion between particles) become important.
Step 5: Conclude that because of these forces and the volume of particles, the ideal gas law does not accurately describe the behavior of gases.
