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 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 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 Waal constants of two gases are as follows : Which of them is more easily liquefiable and which has greater molecular size?

The van der Waals constant for gases A , B , and C are as follows Which gas has the largest molecular volume?

The van der Waals parameters for gases W, X, Y and Z are {:("Gas",a("atm"L^(2)mol^(-2)),b(L"mol"^(-1))),(W," "4.0," "0.027),(X," "8.0," "0.030),(Y," "6.0," "0.032),(Z," "12.0," "0.027):} Which one of these gases has the highest critical temperature?

The van der Waals parameters for gases W, X, Y and Z are {:("Gas",a("atm"L^(2)mol^(-2)),b(L"mol"^(-1))),(W," "4.0," "0.027),(X," "8.0," "0.030),(Y," "6.0," "0.032),(Z," "12.0," "0.027):} Which one of these gases has the highest critical temperature?

The van der Waals' constants of a gas are a=0.687dm^2mol^(-2)b=0.0226dm^3mol^(-1)

van der Waal's constants of two gases X and Y are as given: {:(,a ("litre - atom " mol^(-2)),b ("litre " mol^(-1)),),("Gas X"," "5.6," "0.065,),("Gas Y"," "5.1," "0.012,):} What is correct about the two gases ?

The van der Waal's constants for a gas are a=1.92 atm L^(2) "mol"^(-2),b=0.06 L "mol"^(-1) . If R = 0.08 L atm K^(-1) "mol"^(-1) , what is the Boyle's temperature (in K) of this gas ?