Compressibility factor for `N_(2)` at `27^(o)C` and `100` atm pressures is `1.66`. Calculate number of moles of `N_(2)` gas required to fill a gas cylinder of `821ml` under these conditions.
`3.5`
`3`
`2.5`
`2`

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.

Calculate the number of moles of 22g of CO_2 gas enclosed in a cylinder.

Calculate the density of SO_2 " at " 27^@C and 1.5 atm pressure.

What is the density of N_(2) gas at 227^(@)C and 5.00 atm pressure? (R= 0.0821 atm K^(-1)mol^(-1))

At 27^(@)C and 2.0 atm pressure, the density of propene gas is :

Two moles of ammonia occupy a volume of 5 L at 27^@C and 9.32 atm pressure. Calculate the compressibility factor of the gas.

The compression factor (compressibility factor) for 1 mol of a van der Waals gas at 0^(@)C and 100 atm pressure is found to be 0.5 . Assuming that the volume of a gas molecule is neligible, calculate the van der Waals constant a .

The compression factor (compressibility factor) for 1 mol of a van der Waals gas at 0^(@)C and 100 atm pressure is found to be 0.5 . Assuming that the volume of a gas molecule is neligible, calculate the van der Waals constant a .

Total number of moles of oxygen atoms in 3 litre O_3 (g) at 27^@C and 8.21 atm are :

The pressure of a gas is 2.5 atm . Calculate the value in torr.