Since gases can be highly compressed, what must be true of the spaces between the molecules of the gas?
To understand what must be true of the spaces between the molecules of a gas, we need to consider the properties of gases at the molecular level.
Gases are made up of individual particles known as molecules. These molecules are in constant, random motion and are separated by spaces. The characteristics of these spaces and the interactions between gas molecules determine the behavior of gases.
In the case of highly compressible gases, the spaces between the molecules must be relatively large. This is because gases are highly compressible compared to liquids or solids. When a gas is compressed, its volume decreases, and the molecules come closer together.
The compressibility of gases can be explained by the fact that gas molecules have weak intermolecular forces compared to liquids and solids. These intermolecular forces are the attractive forces between molecules. In gases, the intermolecular forces are relatively weak, leading to larger spaces between the molecules.
When external pressure is applied to a gas, it can be compressed because the weak intermolecular forces allow the gas molecules to be squeezed closer together. As a result, the spaces between the molecules become smaller, and the volume of the gas decreases.
In summary, the spaces between the molecules of a gas must be relatively large to allow for high compressibility. This is because gas molecules have weak intermolecular forces, which enable them to be compressed and occupy smaller volumes.