Gas particles are in constant, random motion. They move in straight lines until they collide with other
particles or the container walls.
Gas particles are much smaller than the distances between them. This implies that the volume occupied by
the particles themselves is negligible compared to the total volume of the gas.
Collisions between gas particles are perfectly elastic. This means that no energy is lost during
collisions, and the total kinetic energy of the system remains constant.
Gas particles do not exert attractive or repulsive forces on each other. This assumption simplifies the
model by neglecting intermolecular forces, which are important in real gases, especially at low
temperatures and high pressures.
The average kinetic energy of gas particles is directly proportional to the absolute temperature. This
means that as temperature increases, the average speed of the gas particles increases, and vice versa.