Question

What property or properties of gases can you point to that support the assumption that most of the volume in a gas is empty space?

Short answer

The compressibility and low density of gases support the assumption that most of the volume in a gas is empty space. Gases are highly compressible due to the considerable empty space between gas particles, allowing their volume to be significantly reduced when pressure is applied. Additionally, gases have a low density compared to solids and liquids because the large empty spaces between particles cause the gas to occupy more volume, reducing its overall density.

Step-by-step solution

Define the properties of gases

Gases have certain unique properties compared to solids and liquids, such as being highly compressible and having a low density. This is due to the particles in a gas being farther apart than in solids or liquids, making empty space between them more significant.

Compressibility of gases

Gases are highly compressible, which means that their volume can be significantly reduced by applying pressure. This compressibility is a result of the considerable empty space between the gas particles. If there were no or little empty space, gas particles would be tightly packed together, and a gas would not be easily compressible.

Low density of gases

Gases have a lower density compared to solids and liquids, mainly because gas particles are farther apart from each other, with lots of empty space between them. The mass of gas particles is the same as in solids and liquids, but the large empty spaces make a gas occupy more volume, reducing its overall density.

Conclusion

The properties of gases, such as their compressibility and low density, support the assumption that most of the volume in a gas is empty space. The considerable empty space between gas particles allows them to be compressed and accounts for their low density compared to solids and liquids, signifying that much of a gas's volume consists of empty space.

Key concepts

Compressibility of gases

The compressibility of gases is a fascinating property that allows them to be easily squeezed or compressed into a smaller volume. This unique characteristic stems from the large amounts of empty space present between the gas molecules. Unlike solids and liquids, where particles are tightly packed, gas molecules are spread out and have significant gaps between them. This ample space makes it possible for gas molecules to move closer together when pressure is applied.
Compressibility is a key feature that distinguishes gases from other states of matter and explains many of their behaviors. For instance, when you inflate a balloon, you are compressing air molecules into a smaller space. If gases were not compressible, inflating a balloon would be much more difficult. The compressibility also plays a crucial role in applications such as

• industrial gas storage
• cooking with gas
• air conditioning systems

Safely storing large volumes of gas in small containers would not be possible without this property. Thus, understanding gas compressibility can help explain why gases can occupy spaces of varying sizes.

Density of gases

The density of gases is generally much lower than that of solids and liquids, primarily due to the vast empty spaces between the particles in a gas. Density is defined as the mass per unit volume, and in gases, the particles are spread out over a larger volume leading to a lower density.
This difference in density is easy to observe in everyday life. For instance, if you compare a balloon filled with air to a stone of the same size, the balloon will float and be lighter because it has less mass in the same amount of space — showcasing the lower density of gases.
The low density of gases has a few practical implications:

• It allows hot air balloons to float, as hot air is less dense than the cooler air outside the balloon.
• It facilitates efficient gas diffusion, enabling gases to mix quickly and evenly.
• It is important in scientific and industrial processes, where the separation and measurement of gases depend on their density differences.

Understanding this concept helps explain why gases often take up more space than they seem to have mass.

Volume of gases

Volume is a determining factor in understanding gases, as they can expand to fill the container they are in, exhibiting no fixed shape or volume. This is largely a result of the particles in gases being in constant, rapid motion and having enough energy to overcome attractions between them.
A key point about the volume of gases is demonstrated by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when temperature is held constant. Mathematically, this is expressed as:\[ P_1V_1 = P_2V_2 \]where \(P_1\) and \(V_1\) represent the initial pressure and volume, while \(P_2\) and \(V_2\) are the final pressure and volume.
Gases adapt to the volume of their container for several reasons:

• They have high kinetic energy, causing them to move and spread out evenly in the available space.
• The random motion of gas molecules means they will naturally disperse until uniformly distributed.
• The lack of strong forces between gas particles allows them to change and adapt their volume easily.

These behaviors highlight the adaptable nature of gases and their ability to occupy any volume offered by their environment.