10 litre container contains He at 210 atm and 300K. Given value of 'b' for 'He' is 0.8 `dm^(3)"mol"^(-1)` Compressibility factor is `(R=0.08"atm" L "mol"^(-1)//K^(-1))`

The density of vapours of a substance of molar mass 18 g at 1 atm pressure and 500 K is 0.36 kg m^(-3) . The value of compressibility factor Z for the vapours will be (Take R = 0.082 L atm mol ^(-1) K^(-1)

80 gm of SO_(x) gas occupies 15 litre at 2atm and 300K. The value of x is : (Given: R= 0.08 L-atm/K-mole)

The volume to be excluded due to only two molecules of a gas in collision with a fixed point of impact is 0.09 l mol^(-1) . If the value of 'a' is 3.6 atm L^(2) mol^(-2) , Calculate Boyle temperature. (R = 0.08 L atm K^(-1) m^(-1) )

PCl_(5)(g) density (in g/L) of mixture at 24 atm and 300 K , when PCl_(5)(g) undergo 50 % decomposition. [R = 0.08 "atm L mol"^(-1) K^(-1)]

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) is

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) is

A 10L flask at 300K contains a gaseous mixture of CO and CO_(2) at a total pressure of 2.0 atm. If 0.2 mol of CO is present, the partial pressure of CO_(2) is ( Use R = 0.082 atm mol^(-1) K^(-1) )

The osmotic pressure of 0.2 molar solution of urea at 300 K(R = 0.082) litre atm mol^(-1)K^(-1) is

A solution containing 3.56 g of a polymer in 1 litre of a solvent was found to have an osmotic pressure of 5.2xx10^(-4) atmosphere at 300K . The molecules mass of the ploymer is ______. (R=0.082 L atm mol ^(-1)K^(-1))