For a real gas (mol.mass =60) if density at critical point is `0.80g//cm^(-3)` and its `T_(c)=(4xx10^(5))/(821)K,` then van der Waals' constant a ( in atm `L^(2)mol^(-2)`) is

For a real gas (mol. Mass= 30 ) if density at critical point is 0.40 g//cm^(3) and its T_(c ) = ( 2 xx 10^(5))/( 821) K, then calculate Vander Waal's constant a( in atm L^(2) mol^(-2)) .

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

The third virial coefficient of a real gas 2xx10^(-2) (L//"mol")^(2) . The value of van der Waals' constant 'b' is:

Calculate the critical constants of a gas whose van der Waals constants are : a=0.751" L"^(2)" atm "mol^(-2) and b=0.0226" L mol"^(-1) .

1 mole of a ciatomic gas present in 10 L vessel at certain temperature exert a pressure of 0.96 atm. Under similar conditions an ideal gas exerted 1.0 atm pressure. If volume of gas molecule is negligible, then find the value of van der Waals' constant ''a'' (in atm L^(2)//mol^(2) ).

1 mole of a ciatomic gas present in 10 L vessel at certain temperature exert a pressure of 0.96 atm. Under similar conditions an ideal gas exerted 1.0 atm pressure. If volume of gas molecule is negligible, then find the value of van der Waals' constant ''a'' (in atm L^(2)//mol^(2) ).

1 mole of a diatomic gas present in 10 L vessel at certain temperature exert a pressure of 0.96 atm. Under similar conditions an ideal gas exerted 1.0 atm pressure. If volume of gas molecule is negligible, then find the value of van der Waals' constant ''a'' (in atm L^(2)//mol^(2) ).