Density of hydrogen gas at `27^(@)C` is 0.25g/lt .If van der waals gas constant 'b',f or `H_(2)` is 0.5lt/mol ,then compressibility factor of `H_(2)` is

Compressibility factor for H_(2) behaving as real gas is

The van der Waals' constant 'a' for CO_(2) gas is greater than that of H_(2) gas. Its mean that the

Compressibility factor for H2 behaving as real gas is

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

The van der Waals equation for one mol of CO_(2) gas at low pressure will be

The van der Waals equation for one mol of CO_(2) gas at low pressure will be

At low pressure the van der Waals' equation is reduced to [P +(a)/(V^(2)]]V =RT The compressibility factor can be given as .

Isothermally at 27^(@) C, one mole of a van der Waals gas expands reversibly from 2 litres to 20 litres. Calculate the work done.

The critical pressure P_(C) and critical temperature T_(C) for a gas obeying van der Waal's equation are 80 atm at 87^(@) C. molar mass of the gas is 130 g/mole. The compressibility factor for the above gas will be smaller than unity under the following condition:

The van der Waals constant ‘b’ for oxygen is 0.0318 L mol^(-1) . Calculate the diameter of the oxygen molecule.