Question

1. what is true of all particles of gas enclosed within a container?

they move at different speeds.
they have the same kinetic energy.
they never collide with each other.

Explanation:

According to the kinetic - molecular theory of gases:

• Gas particles are in constant random motion and do collide with each other (so the option "They never collide with each other" is wrong).
• The average kinetic energy of gas particles is related to the temperature. Different particles (with different masses) in the same gas sample (at the same temperature) will have different speeds because \(KE=\frac{1}{2}mv^{2}\). If \(KE\) (average, related to temperature) is the same for a gas sample (same \(T\)), but \(m\) (mass of particles) can be considered as the same for a pure gas (or for a mixture, the concept of average molar mass), but in general, particles move at different speeds. The statement "They have the same kinetic energy" is incorrect in a strict sense as it's the average kinetic energy that is related to temperature. The most accurate is that gas particles move at different speeds.

Answer:

They move at different speeds.