Comperessibility factor `(Z)` for `N_(2)` at `-50^(@) C` and 800 atm pressure is 1.95 Calculate mole of `N_(2)` gas required to fill a gas cylinder of `100mL` capacity under the given conditions .

Compressibility factor (Z) for N_(2)" at "-50^(@)C and 800 atm pressure is 1.95 calculate mole of N_(2) gas required to fill a gas cylinder of 100 L capacity under the given conditions.

The compressibility factor for a given real gas is 0.927 at 273 K and 100 atm Calculate the amount of gas required to fill a gas cylinder of 100 litre capacity under given conditions (Mol weight of gas =30) .

At 273.15K and under a pressure of 10.1325 Mpa, the compressibility factor of O_(2) is 0.927. Calcualte the mass of O_(2) necessary to fill a gas cylinder of 100 dm^(3) capacity under the given conditions.

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) ] ?

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.

Nitrogen gas is filled in a container of volume 2.32 L at 32^@C and 4.7 atm pressure . Calculate the number of moles of gas .