Question

Which of the following is true for a gas under conditions of very low temperature?

PV > nRT, because the actual volume of the gas would be more than its ideal value.
PV < nRT, because the volume is smaller due to significant intermolecular force effects.
PV = nRT, because the actual volume of the gas molecules becomes considerable.
PV = nRT, because all gases behave ideally at very low temperatures.

Answer 1

D)

Step-by-step explanation:

PV/nRT=1, because particles are unable to overcome intermolecular attractions

Answer 2

PV < nRT, because the volume is smaller due to significant intermolecular force effects.

Step-by-step explanation:

FLVS exam states that this is correct because gasses change their "ideal" behaviors at lower temperatures.