The van der waals constant 'a' for different gases are given below :
`{:("Gas",""a("atm lit"^(-2)"mol"^(-2))),(O_(2)" ",1.36),(N_(2),1.39),(CH_(4),2.25),(NH_(3),4.17):}`
The gas that can be most easily liquefied is

The Van der Waals constants for two gases A and B are as follows : {:("Gas",a("atm L"^(2)" mol"^(-2)),b("L mol"^(-1))),(" A"," 1.63"," 0.0326"),(" B"," 3,72"," 0.0521"):} Which of these (i) is more easily liquefied? (ii) has larger molecular size?

The van der Waals constants for two gases are as follows : {:("Gas",a(atm L^(2)mol^(-2)),b(L Mol^(-1))),(X,1.39,0.0391),(Y,3.59,0.0427):} Which of them is more easily liquefiable and which has greater molecular size ?

The van der Waals' constant 'a' for CO_(2) gas is greater than that of H_(2) gas. Its mean that the

Boyle temperature of vaiour gases are given below : {:("Gas",T_(B)(K),),(H_(2),117,),(He,23,),(CH_(4),498,),(O_(2),406,):} Which gas can be liquefied most easily ?

The values of the van der Waals' constant a for some gases are given below. H_2 = 0.245 " atm " L^2 mol^(-2) O_2 = 1.360 " atm " L^2 mol^(-2) CO_2 = 3.590 " atm " L^2 mol^(-2) NH_3 = 4.170 " atm " L^2 mol^(-2) Arrange these gases in the decreasing order of their liquefaction tendencies.

The van der Waals' constant 'a' for the gases O_(2), N_(2), NH_(3) "and " CH_(4) are 1.36, 1.39, 4.17 and 2.253 respectively, the gas which can be most easily liquefied is :

The van der Waals' constant 'a' for the gases O_(2), N_(2), NH_(3) "and " CH_(4) are 1.36, 1.39, 4.17 and 2.253 respectively, the gas which can be most easily liquefied is :