For one mole of a van der Waals' gas when `b=0` and `T=300K`, the `pV vs 1//V` plot is shown below. The value of the vander Waals' constant `a`(atm `L mol^(-2)`)

For one mole of a van der Waals’ gas when b = 0and T =300 K, the pV vs. 1/V plot is shown below. The value of the van der Waals’ constant a (atm L mol^(-2) ) is

For one mole of a van der Waals gas when b =0 and T =30 K the PV vs1//V plot is shown below The value of the van Waals constant a ("atm litre"^(2) mol^(-2)) is .

For one mole of a van der Waals gas when b = 0 and T = 300 K , the PV vs 1/V plot is shown below . The value of the van der Waals constant a (atm "litre"^(2) mol^(-2) ) is

The compressibility factor for definite amount of van der Waals' gas at 0^(@)C and 100 atm is found to be 0.5 . Assuming the volume of gas molecules negligible, the van der Waals' constant a for gas is

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the significance of van der Waals constant 'a'?

Compressibility factor for 1 mole of a van er waals gas at 0^(@)C and 100 atms pressure is 0.5 assuming that volume of a gas molecule is negligible, calculate the van der waals constant, a.

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the value of Z for an ideal gas?