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.

The number of molecules 67.2 L of a gas at 0^@C and 1 atm pressure is:

The compressibility factor (Z) of one mole of a van der Waals gas of negligible ‘a’ value is

The compresibility factor (Z) of one mole of a van der waals gas of negligible 'a' value is-

Compressibility factor of 2 mol of NH_(3) gas at 27^(@)C and 9.18 atm pressure is 0.931. if the volume of the gas molecules is not taken into consideration, then what is the value of van der waals constant 'a' for NH_(3) gas?

What property of molecules of real gases is indicated by van der Waal’s constant ‘a’?

At constant temperature and pressure, the compressbility factor (Z) for one mole of a van der waals gas is 0.5. if the volumes of the gas molecules are considered to negligible, then show that a=(1)/(2)V_(m)RT , where V_(m) and T are the molar volume and temperature of the gas respectively.

Compressibility factor of a real gas at 0^(@)C and 100 atm pressure is 0.927. at this temperature and pressure, how much of this real gas is required to fill a vessel of 100 L [molar mass= 40g*mol^(-1) ] ?

Calculate the work done when 1 mol of water vaporises at 100^(@)C and 1 atm pressure. Assume water vapour behaves like an ideal gas.

Which of the following is the unit of van der waals gas constant b-

if Z is a compressibility factor, van der waals equation at low pressures can be written as