A sample of impure air contains 80% `N_(2)`, 10% `O_(2)` 5% `CO_(2)` and 5% Ar by volume. The average (At wt. of Ar = 40)

A sample of impure air contains 80% N_(2) . 10% 5% CO_(2) and 5% Ar by volume. The average molecular weight of the sample is : [Ar=40]

A gaseous mixture contains 40% O_(2), 40% N_(2), 10% CO_(2), 10% CH_(4) by volume. Calculate the vapour density of the gaseous mixture.

A gaseous mixture contains 40% O_(2), 40% N_(2), 10% CO_(2), 10% CH_(4) by volume. Calculate the vapour density of the gaseous mixture.

Atmospheric air has 78 % N_(2) , 21 % O_(2) , 0.9 % Ar and 0.1 % CO_(2) by volume. What is the molecular mass of air in the atmosphere ?

If the components of air are N_(2), 78%, O_(2), 21%, Ar, 0-9% and CO_(2), 0-1% by volume, what would be the molecular weight of air?

The air contain 80% N_(2) and 20% O_(2) by volume. The volume occupied by 40 gm air at 27^(@)C and 760 mm Hg pressure approximately. [Given: R=0.08atm-litre- "mol"^(-1)K^(-1) ]

Average molecular weight of a gaeous mixture which contains 80% by mole N_(2) & rest O_(2) gas is-