# Problem: What are each of the following observations an example of?Drag the appropriate items to their respective bins.There is a gas leak in the kitchen and you smell gas in the bedroom after 10 minutes.When there is a leak in the gas cylinder the pressure of gas decreases slowly over time.When a small hole is made in the top of a coke bottle the carbon dioxide gas moves out of the bottle over time.Hair spray applied in the bedroom can be smelled in the hallway a short time later.The kinetic molecular theory of gases explains how gas molecules behave in terms of motion, speed, and energy.One important aspect of this theory deals with the relationship between temperature and the average speed of the gas molecules. Increasing the temperature of a gas sample increases the average kinetic energy of the molecules. The kinetic energy of a molecule determines its speed. It is important to realize that not all molecules in a sample will have the same kinetic energy, which is why we refer to the average kinetic energy and the average speed. The speed of a particle with average kinetic energy is called the root mean square (rms) speed, vrms.The rms speed may be expressed by the following equation:vrms=3RTMwhere R is the ideal gas constant, T is the absolute temperature, and M is the molar mass of the substance in kilograms per mole.The constant motion of gas molecules causes diffusion and effusion. Diffusion is the gradual mixing of two substances resulting from the movement of their particles. Effusion is the gradual escape of gas molecules through microscopic holes in their container.

###### Problem Details

What are each of the following observations an example of?

Drag the appropriate items to their respective bins.

There is a gas leak in the kitchen and you smell gas in the bedroom after 10 minutes.
When there is a leak in the gas cylinder the pressure of gas decreases slowly over time.
When a small hole is made in the top of a coke bottle the carbon dioxide gas moves out of the bottle over time.
Hair spray applied in the bedroom can be smelled in the hallway a short time later.

The kinetic molecular theory of gases explains how gas molecules behave in terms of motion, speed, and energy.

One important aspect of this theory deals with the relationship between temperature and the average speed of the gas molecules. Increasing the temperature of a gas sample increases the average kinetic energy of the molecules. The kinetic energy of a molecule determines its speed. It is important to realize that not all molecules in a sample will have the same kinetic energy, which is why we refer to the average kinetic energy and the average speed. The speed of a particle with average kinetic energy is called the root mean square (rms) speed, vrms.

The rms speed may be expressed by the following equation:

${\mathbf{v}}_{\mathbf{rms}}\mathbf{=}\sqrt{\frac{\mathbf{3}\mathbf{RT}}{\mathbf{M}}}$

where R is the ideal gas constant, T is the absolute temperature, and M is the molar mass of the substance in kilograms per mole.

The constant motion of gas molecules causes diffusion and effusion. Diffusion is the gradual mixing of two substances resulting from the movement of their particles. Effusion is the gradual escape of gas molecules through microscopic holes in their container.