what do we assume about volume of the actual molecules themselves in a sample of gas, compared to the bulk volume overall?why?
When considering the volume of a sample of gas, we assume that the volume of the actual molecules themselves is negligible compared to the bulk volume of the gas. This assumption is based on the Kinetic Molecular Theory of Gases.
The Kinetic Molecular Theory states that gases are composed of tiny particles, such as atoms or molecules, that are in constant motion and have negligible volume compared to the total volume of the gas. These particles occupy so little space relative to the entire volume of the gas that we can consider them to have no significant size.
In reality, gas molecules do have some volume, but it is so small compared to the space between them that it is typically considered insignificant. Essentially, the particles are assumed to behave as point masses, occupying no physical space. This assumption simplifies the mathematical treatment of gases and makes it easier to study their properties.
Therefore, when calculating the volume of a gas sample, we only consider the amount of space that the gas occupies as a whole, without accounting for the individual volume of the molecules.