Question

Our model of an ideal gas describes gases as a collection of small, rigid spheres, in constant, rapid motion. Because the molecules are very small compared to the space they occupy, we say the molecules have negligible volume. This means that molecules are more likely to collide with the container walls than they are to collide with each other.
Nonetheless, intermolecules collisions are possible and do occur. We refer to the distance a molecule can travel without hitting something else as its mean free path.
Which of the following change possibilities would INCREASE the mean free path of molecules is a sample of confined gas, assuming no change in the number of molecules in the system?

• A. An increase in pressure at constant temperature.
• B. An increase in temperature at constant pressure.
• C. An increase in temperature at constant volume.
• D. An increase in pressure at constant volume.

Answer 1

The correct option is B An increase in temperature at constant pressure.

Mean free path is the average distance a molecule travels, before colliding with another molecule. So, as the temperature increases Kinetic energy of the molecules increases Faster motion of molecules take place within the same time interval.Therefore, Mean free path increases with increase Temperature.