The van der Waals equation for one mole of a real gas can be written as `(P+(a)/(v^(2))(V-b)=RT`. For the gases `H_(2), NH_(3), and CH_(4)`, the value of 'a' `"bar L"^(-2)"mol"^(-2)` are 0.2453, 4.170 and 2.253` respectively.
Which of the following can be inferred from the 'a' values?

The unit of the van der Waals gas equation parameter 'a' in (P+(an^(2))/(V^(2)))(V-nb)=nRT is :

The van der Waals, equation for n moles of real gas is: (P+(n^(2)a)/(V^(2)))(V - nb) = nRT where P is the pressure, V is the volume , T is the absolute temperature, R is the molar gas constant and a, b are van der Waal's constant. Which of the following have the same dimension as those of PV ?

The van der Waal's equation of state for some gases can be expressed as : (P + (a)/( V^(2))) ( V - b) = RT Where P is the pressure , V is the molar volume , and T is the absolute temperature of the given sample of gas and a, b , and R are constants. Which of the following does not have the same dimensional formula as that for RT?

The van der Waal's equation of state for some gases can be expressed as : (P + (a)/( V^(2))) ( V - b) = RT Where P is the pressure , V is the molar volume , and T is the absolute temperature of the given sample of gas and a, b , and R are constants. Which of the following does not have the same dimensional formula as that for RT?

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 :

van der Waal's equation of state for real gases may be written as: PV_(m)=RT(1+(B)/(V_(m))+(C)/(V_(m)^(2))+....) Select the correct statement(s).