Question

Imagine the movement of gas particles in a closed container. According to the kinetic molecular theory, which statements below are true of the gas particles? Check all that apply.

Gas particles act like tiny, solid spheres.

Gas particles are in constant, random motion.

Gas particles at lower temperatures move faster.

Collisions are elastic, there is no energy lost as the particle hits the sides of the container.

Slower moving particles collide more often and with more force with the container.

Answer 1

True:
- Gas particles act like tiny, solid spheres. — True in the KMT/ideal-gas model: particles are treated as small, hard (rigid) spheres with negligible volume and no internal structure.
- Gas particles are in constant, random motion. — True: they move rapidly and randomly in all directions.
- Collisions are elastic, there is no energy lost as the particle hits the sides of the container. — True (ideal assumption): collisions conserve kinetic energy (energy can be exchanged but not lost).

False:
- Gas particles at lower temperatures move faster. — False: lower temperature → lower average kinetic energy → slower average speeds.
- Slower moving particles collide more often and with more force with the container. — False: faster particles hit the walls more frequently and deliver greater momentum change per collision, so they collide more often and with more force.