1023 molecules of nitrogen, argon and carbon dioxide each are confined in three closed boxes of a large fixed volume V, at the same temperature T. Knowing the molecular weights of the gases are in the order MCO2>MN2>MAr, what can you say about the pressures of the gases in each container?
At low densities, all real gases seem to obey the ideal gas equation PV=nRT.
This suggests, at constant volume, quantity, and temperature, P=(nRTv) will be same for all gases.
∴ In our discussion, PAr=PN2=PCO2.
The molecular masses won't play any real role at low densities