Question

Which of the following is true for a gas under conditions of very high pressure? (5

points)
1) PV > nRT, because the real volume of the gas would be more than the ideal
volume.
2) PV = nRT, because intermolecular forces are considerable at very high
pressures.
3) PV = nRT, because all gases behave as ideal gases at very high pressures.
04) PV = nRT, because the volume of the gas would become negligible.

Answer 1

1) PV > nRT, because the real volume of the gas would be more than the ideal volume.

Step-by-step explanation:

just took the test :)

Answer 2

1) PV > nRT, because the real volume of the gas would be more than the ideal

volume.

Step-by-step explanation:

According to the ideal gas equation; PV = nRT. Let us recall that this equation only holds under ideal conditions.

Gases exhibit ideal behavior under high temperature and low pressure. At higher pressure, the real volume of the gas is larger than the ideal volume of the gas.

Thus, at high pressure, PV > nRT, because the real volume of the gas would be more than the ideal volume.