# 7.4.1: Practice Problems- Kinetic Molecular Theory

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PROBLEM $$\PageIndex{1}$$

Using the postulates of the kinetic molecular theory, explain why a gas uniformly fills a container of any shape.

The first three parts of Kinetic Molecular Theory explain this:

Gases are composed of molecules that are in continuous motion, travelling in straight lines and changing direction only when they collide with other molecules or with the walls of a container.

The molecules composing the gas are negligibly small compared to the distances between them.

The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls.

PROBLEM $$\PageIndex{2}$$

Can the speed of a given molecule in a gas double at constant temperature? Explain your answer.

Yes. At any given instant, there are a range of values of molecular speeds in a sample of gas. Any single molecule can speed up or slow down as it collides with other molecules. The average velocity of all the molecules is constant at constant temperature.

PROBLEM $$\PageIndex{3}$$

Describe what happens to the average kinetic energy of ideal gas molecules when the conditions are changed as follows:

1. The pressure of the gas is increased by reducing the volume at constant temperature.
2. The pressure of the gas is increased by increasing the temperature at constant volume.
3. The average velocity of the molecules is increased by a factor of 2.

Kinetic energy will not change (temperature is unchanged)

Kinetic energy will increase (temperature is increased)

The kinetic energy will increase by a factor of four (velocity is squared in the equation)

PROBLEM $$\PageIndex{4}$$

The distribution of molecular velocities in a sample of helium is shown in the photo below (Figure 7.4.4). If the sample is cooled, will the distribution of velocities look more like that of H2 or of H2O? Explain your answer.