`1 mol` of `C Cl_(4)` vapours at `77^(@)C` occupies a volume of `35.0 L`. If van der Waals constants are `a=20.39 L^(2) atm mol^(-2)` and `b=0.1383 L mol^(-1)`, calculate compressibility factor `Z` under
(`a`) Low pressure region
(`b`) High pressure region

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) .

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

2 mol of a van der waals gas at 27^(@)C occupies a volume of 20 L. what is the pressure of the gas? [a=6.5 atm*L^(-2)*mol^(-2),b=0.056L*mol^(-1) ]

The values of the van der Waals constants for a gas a = 4.10 dm^(6) "bar" mol^(-2) and b = 0.035 dm^(3) mol^(-1) . Calculate the values of the critical temperature and critical pressure for the gas.

The values of the van der Waals constants for a gas a = 4.10 dm^(6) "bar" mol^(-2) and b = 0.035 dm^(3) mol^(-1) . Calculate the values of the critical temperature and critical pressure for the gas.

The inversion temperature Ti(K) of hydrogen is (Given van der Waal’s constant a and b are 0.244 atm L^2 mol^(-2) and 0.027 L mol^(-1) respectively.)

Assuming CO_(2) to be van der Waals gas, calculate its Boyle temperature. Given a=3.59" L"^(2)" atm " mol^(-2) and b=0.0427" L "mol^(-1) .

2 moles of ammonia occupied a volume of 5 lit at 27^@C . Calculate the pressure if a=4.17atmL^2 mol^(-2), b= 0.0371 L mol^(-1)

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at 37^(@)C . Given that the van der Waal’s constants are a = 3.59 L^(2) " atm "mol^(-2) and b = 0.0427 L mol^(-1) . Compare the value with the calculated value if the gas were considered as ideal.