A real gas most closely approaches ideal behavior under which of the following conditions?

Calculate the pressure in bar exerted by 128 g of oxygen gas contained in a 20.0 L vessel at a temperature of $27^\circ C$, assuming ideal gas behavior. (Use $R = 0.0831\ L\ bar\ K^{-1}\ mol^{-1}$)

When air is blown to balloon (at constant temperature) its pressure and volume both increases. This violates:

At what temperature will the average kinetic energy of gas molecules be double its value at 27°C?

An ideal gas expands according to $PV =$ constant. On expansion, the temperature of gas:

Pressure remaining constant, the volume of a given sample of gas at 127\,^\circ C will be doubled at:

If volume containing gas is compressed to half, how many moles of gas remained in the vessel?

The density of ${N_2}$ gas at 0.821 atmospheric pressure and ${7^0}C$

When a sample of gas is compressed at constant temperature from 15 atm to 60 atm, its volume changes from $76\,\,{\rm{c}}{{\rm{m}}^3}\,\,{\rm{to}}\,\,20.5\,\,{\rm{c}}{{\rm{m}}^3}$. Which of the following statements are possible explanations of this behaviour? 1. The gas behaves non-ideally. 2. The gas dimerises. 3. The gas is absorbed into the vessel walls.

A real gas most closely approaches ideal behavior under which of the following conditions?

To raise the volume of a gas by four times, the following method may be adopted. Which of the method is wrong?