The density of a mixture of `N_(2)` and `O_(2)` at `NTP` is `1.3gL^(-1)`.Calculate partial pressure of `O_(2)` .(in atm)

Partial pressure of O_2 in alveoli is

If the density of a mixture of O_(2)&N_(2) at N.T.P. is 1.258 g//l. The partial volume of O_(2) in 3 mole of mixture is

Density of dry air ( only N_(2) and O_(2)) is 1.24g litre^(-1) at 760 m m and 300 K . Find the partial pressure of N_(2) gas in aire. ( Take R=(1)/(12) litre litre atm // mol K, mol. Wt. of N_(2) =28)

The vapour density of a mixture containing N_(2) (g) and O_(2) (g) is 14.4. The percentage of N_(2) in the mixture is :

In a ten litre vessel, the total pressure of a gaseous mixture containing H_(2), N_(2) and CO_(2) is 9.8atm. The partial pressures of H_(2) and N_(2) are 3.7 and 4.2 atm respectively. Then the partial pressure of CO_(2) is

The density of an equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm and 373.5K is 2.0 g/L. Calculate K_(C) for the reaction N_(2)O_(2)(g) iff 2NO_(2)(g)

A sample of air contains only N_(2), O_(2) and H_(2)O . It is saturated with water vapours and the total pressure is 640 torr. The vapurs of water is 40 torr and the molar ratio of N_(2) : O_(2) is 3 : 1 . The partial pressure of N_(2) in the sample is

Vapour density of mixture of NO_(2) and N_(2) O_(4) is 34.5 , then percentage abundance of NO_(2) in mixture is

The density of an equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm is 3.62 g L^(-1) at 288 K and 1.84 g L^(-1) at 348 K . Calculate the entropy change during the reaction at 348 K .

Density of equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm and 384 K is 1.84 g dm^(-3) . Calculate the equilibrium constant of the reaction. N_(2)O_(4)hArr2NO_(2)