Question

At a specific temperature and volume, which gas, Ar or CCl₄, would you anticipate to exhibit a greater deviation from ideal behavior in terms of pressure? Explain why.

Answer 1

Real gases deviate from ideal behavior at high pressures and low temperatures due to measurable volumes and intermolecular interactions.

Step-by-step explanation:

At high pressures and low temperatures, gases deviate from ideal behavior due to the two basic assumptions behind the ideal gas law no longer being valid. Real gases have measurable volumes and intermolecular interactions become significant under these conditions.

As a result, the total volume occupied by the gas becomes greater than predicted by the ideal gas law.

In the given scenario, the gas that is more likely to exhibit a greater deviation from ideal behavior in terms of pressure would be CCl₄. This is because CCl₄ is a larger molecule compared to Ar, and therefore its volume is more significant compared to the volume of the container at high pressures.

As a result, the pressure measured for CCl₄ would be higher than the pressure predicted by the ideal gas law.CCl₄ is likely to exhibit a greater deviation from ideal behavior in terms of pressure compared to Ar.