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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.

Respuesta :

Hardy007

Answer:

D)

Explanation:

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

Answer:

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

Explanation:

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