Question

recall the postulates of kinetic - molecular theory. read the list and check all the statements that apply to the behavior of an ideal gas: gas particles behave like hard spheres gas particles travel randomly gas particles are attracted to each other energy is lost when gas particles collide average kinetic energy of a collection of gas particles depends on the temperature gas particles occupy most of the space within a container gas particles have mass and volume done

Explanation:

• According to the kinetic - molecular theory of ideal gases:
• Gas particles are considered as hard spheres (no deformation during collisions).
• They travel in random straight - line paths.
• The average kinetic energy of gas particles is directly proportional to the absolute temperature ($KE_{avg}=\frac{3}{2}kT$, where $k$ is the Boltzmann constant and $T$ is the temperature).
• There are no attractive or repulsive forces between gas particles (so the statement “gas particles are attracted to each other” is wrong).
• Collisions between gas particles (and between particles and the container walls) are elastic (no energy loss, so “energy is lost when gas particles collide” is wrong).
• Gas particles occupy a negligible volume compared to the volume of the container (so “gas particles occupy most of the space within a container” is wrong).
• In the ideal gas model, gas particles are considered to have mass but no volume (so “gas particles have mass and volume” is wrong in the strict sense of ideal gas theory, although real - gas particles have both mass and volume).

Answer:

• gas particles behave like hard spheres
• gas particles travel randomly
• average kinetic energy of a collection of gas particles depends on the temperature