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 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?

If the Vander Waal's constant of gas A are given as - a ( atm L^(2) mol^(2) ) =6.5 b( L mol^(1) ) 0.056 than critical pressure of A is

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?

Consider the following statements. If the Van der Waal's parameters of two gases are given as :- {:(, a//dm^(6) "bar mol"^(-2), b//dmmol ^(-1)), (Gas A , 6.5, 0.055), (Gas B , 2, 0.01):} (i) Critical volume of A lt Critical volume of B (ii) Critical pressure of A gt Critical pressure of B (iii) Critical temperature of A gt Critical temperature of B Which of the above statements is/are incorrect?