Final answer:
The idea that inter-molecular space among gas molecules is narrow is false. In a gas state, there is a large separation between molecules with negligible intermolecular forces enabling gases to be highly compressible and take on the shape and volume of their container. correct is false.
Step-by-step explanation:
The statement that the inter-molecular space among gas molecules is narrow is false. In a gas state, the molecules or atoms are highly separated, which allows gases to be highly compressible, and the intermolecular forces are minimal which permits gases to take on the shape and volume of their container.
The ideal gas equation assumes that molecules are negligibly small compared to the distance between them. Consequently, intermolecular attractions between gas molecules can be disregarded under certain conditions, like low pressure and high temperature, where gases approach ideal behavior.
However, it is important to acknowledge that the ideal gas behavior is an approximation, and real gases may show deviation from the ideal gas laws, especially at high pressures and low temperatures, where intermolecular forces become more significant.
Figure illustrations in educational materials typically show the molecules in a gas state as widely separated from each other, reinforcing that the intermolecular space in a gas is indeed not narrow.