Under the ideal gas model, the volume occupied by the gas molecules themselves is considered negligible.

Under the ideal gas model, the volume occupied by the gas molecules themselves is considered negligible.

• A. True
• B. False
• C. Not specified
• D. It depends

Answer: (A)

In the ideal gas model, gas molecules are treated as point particles with essentially no volume, and there are no intermolecular forces. Because of that, the space the molecules themselves occupy is negligible compared to the container volume, so the volume in the ideal gas law refers to the container volume available for motion, not the actual size of the molecules. This makes the statement true. In real gases, molecules do have finite size and interactions become important at higher pressures, which is why the ideal model uses this simplification and why corrections like those in the van der Waals equation exist. The other options would imply uncertainty or dependence on conditions, which isn’t part of the ideal gas framework.

In the ideal gas model, gas molecules are treated as point particles with essentially no volume, and there are no intermolecular forces. Because of that, the space the molecules themselves occupy is negligible compared to the container volume, so the volume in the ideal gas law refers to the container volume available for motion, not the actual size of the molecules. This makes the statement true. In real gases, molecules do have finite size and interactions become important at higher pressures, which is why the ideal model uses this simplification and why corrections like those in the van der Waals equation exist. The other options would imply uncertainty or dependence on conditions, which isn’t part of the ideal gas framework.