If we believed that the molecules of a gas move around fairly rapidly, we can use this to explain all of the following EXCEPT

why adding more gas increases the pressure.

why most of the volume of the gas sample is taken up by the gas molecules.

why the gas molecules do not settle out on the bottom of the container.

why gas pressure rises with increasing temperature.

The answers are confusing to me in light of the question; therefore, I've chosen to steer clear.

why most of the volume of the gas sample is taken up by the gas molecules.

Since gases are easily compressed, it follows that most of the volume of the gas sample would be empty space. There is a lot of space between the molecules.

We can use the idea that gas molecules move around rapidly to explain why adding more gas increases the pressure, why most of the volume of the gas sample is taken up by the gas molecules, and why the gas molecules do not settle out on the bottom of the container. However, this concept does not explain why gas pressure rises with increasing temperature. The relationship between gas pressure and temperature is explained by the kinetic theory of gases, which states that an increase in temperature increases the average kinetic energy of gas molecules, leading to an increase in their speed and collisions with the container walls, thereby increasing the pressure.

To determine the answer to this question, we need to consider the given statement and analyze each option provided. The statement suggests that the rapid movement of molecules in a gas can explain certain phenomena. Let's evaluate each option individually:

1. Why adding more gas increases the pressure: This can be explained by the concept of collisions between gas molecules. When more gas molecules are added to a fixed volume, the frequency of collisions increases, leading to more strikes against the container walls. This increased frequency of collisions results in a higher pressure. So, this option can be explained by the rapid movement of gas molecules.

2. Why most of the volume of the gas sample is taken up by the gas molecules: According to the kinetic theory of gases, gas molecules are in constant motion and have negligible volume compared to the spaces between them. This implies that most of the volume of a gas sample is indeed taken up by the gas molecules themselves. Therefore, this option can also be explained by the rapid movement of gas molecules.

3. Why the gas molecules do not settle out on the bottom of the container: This phenomenon can be explained by the random motion of gas molecules. Due to their high speed and constant collisions, gas molecules are quickly mixed throughout the entire container and do not settle at the bottom. Hence, this option is indeed explained by the rapid movement of gas molecules.

4. Why gas pressure rises with increasing temperature: This concept can be explained using the kinetic theory of gases as well. When temperature increases, gas molecules gain kinetic energy and move with greater speed and collide with increased force. Consequently, the frequency and intensity of collisions with the container walls increase, leading to an increase in gas pressure. Therefore, this option is also explained by the rapid movement of gas molecules.

Thus, considering all the options, it appears that the rapid movement of gas molecules can explain all of the provided phenomena. Therefore, the answer is that all of the options can be explained by the rapid movement of gas molecules.