Question

2) If the volume of a gas is greater than you would expect based on the ideal gas law, the best explanation for this is because the.... 3) If the volume of a gas is less that you would expect based on the ideal gas law, the best explanation for this is because the....

Answer 1

If the volume of a gas is greater than expected based on the ideal gas law, it is because the molecules of a real gas have small but measurable volumes. If the volume of a gas is less than expected based on the ideal gas law, it is because the molecules of an ideal gas are assumed to have zero volume.

Step-by-step explanation:

If the volume of a gas is greater than you would expect based on the ideal gas law, the best explanation for this is because the molecules of a real gas have small but measurable volumes. At low pressures, the gaseous molecules are relatively far apart, but as the pressure of the gas increases, the intermolecular distances become smaller and smaller. As a result, the volume occupied by the molecules becomes significant compared with the volume of the container. Consequently, the total volume occupied by the gas is greater than the volume predicted by the ideal gas law.

If the volume of a gas is less than you would expect based on the ideal gas law, the best explanation for this is because the molecules of an ideal gas are assumed to have zero volume. In the ideal gas model, the volume occupied by its atoms and molecules is a negligible fraction of V. Thus, the ideal gas law predicts that the volume of a gas is solely determined by the volume of the container. However, in reality, the molecules of a real gas have small but measurable volumes. Therefore, the total volume occupied by the gas is less than the volume predicted by the ideal gas law.

Answer 2

The best explanation for a gas having a greater volume than expected based on the ideal gas law is because the molecules of a real gas have small but measurable volumes, which become significant at high pressures. Conversely, if the volume of a gas is less than expected, it could be due to low temperatures or high pressures where deviations from ideal behavior are observed.

Step-by-step explanation:

The best explanation for a gas having a greater volume than expected based on the ideal gas law is because the molecules of a real gas have small but measurable volumes, which become significant at high pressures. When the pressure of a gas increases, the intermolecular distances become smaller, causing the volume occupied by the gas molecules to become significant compared to the volume of the container. This leads to the total volume occupied by the gas being greater than the volume predicted by the ideal gas law.

On the other hand, if the volume of a gas is less than expected based on the ideal gas law, it could be because the gas is at very low temperatures or very high pressures, where deviations from ideal behavior are commonly observed. The ideal gas law does not work well under such conditions, causing the actual volume of the gas to be less than predicted by the ideal gas law.