The comperessibility factor for `N_(2) `at `-50^(@) C` and 800 atm pressure is 1.95. The mole of `N_(2)` required to fill up a gas cylinder of 100L capacity are

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 nitrogen at 330K and 800 atm is 1.90 and at 570K and 200 atm is 1.10 . A certain mass of N_(2) occupies a volume of 1dm^(3) at 330K and 800 atm calculate volume occupied by same quantity of N_(2) gas at 570 K and 200 atm

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

The density of O_2 gas at 127^o C and 4.0 atm pressure is (R = 0.082 L atm K^-1 mol^-1 )

What is the compressibility factor (Z) for 0.02 mole of a van der Waals's gas at pressure of 0.1 atm. Assume the size of gas molecules is negligible. Given : RT=20 L atm mol^(-1) and a=1000 atm L^(2) mol^(-2)

A 1 mol gas occupies 2.4L volume at 27^(@) C and 10 atm pressure then it show :-

Pure hydrogen sulphide is stored in a tank of 100 litre capacity at 20^(@) C and 2 atm pressure. The mass of the gas will be

At 1 atm pressure freezing of n mole of water liquid (0^(@)C) then heat transfer:

If the weight of one atom is (16)/(N_(A)) gm and it form X_(2) type gas. How many grams of X_(2) is required to fill up the gas vessel with volume 350 mL at 0^(@)C and to obtain the pressure 2 atm-

What will be the pressure of 14g N_(2) (in atm) present in a 2 litre cylinder at 300K?