Home
Class 11
CHEMISTRY
Calculate the total pressure in a 10 L c...

Calculate the total pressure in a 10 L cylinder which contains 0.4 g of helium, 1.6 g of oxygen and 1.4 g of nitrogen at `27^(@)`C. Also calculate the partial pressures of He gas in the cylinder. Assume Ideal behaviour for gases.
R = 0.082 L atm `k^(-1) mol^(-1)`

Text Solution

Verified by Experts

`p_("total") = 0.4926` atm
`p_(He) = 0.2463` atm
`p_(O_(2)) = 0.1231` atm
`p_(N_(2)) =0.123` atm
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the total pressure in a 10 L cylinder which contains 0.4 g helium ,1.6 of oxygen and 1.4 g nitrogen at 27^(@)C . Also calculate the partial of helium gas in the cylinder. Assume ideal hehaviour for gases.

3.2 g of oxygen and 0.2 g of hydrogen are placed in a 1.12 L flask at 0^(@)C . The total pressure of the gas mixture will be

The partial pressure of ethane over a solution containing 6.56 xx 10^(-2) g of ethane is 1 bar. If the solution contains 5.0 xx 10^(-2) g of ethane, then what will be the partial pressure of the gas?

2.8 g of N_(2) , 0.40 g of H_(2) and 6.4g of O_(2) are placed in a container of 1.0 L capacity at 27^(@)C . The total pressure in the container is :

The osmotic pressure of a solution containing 40 g of solute ("molecular mass 246") per litre at 27^(@)C is (R=0.0822 atm L mol^(-1))

A hydrocarbon contains 10.5 g of carbon per gram of hydrogen. 1 L of vapour of the hydrocarbon at 127^(@)C and 1 atm pressure weighs 2.8 g . Find the molecular formula of the hydrocarbon.

Blood freezes at 272.44 K and a solution of 3.0 g of urea in 250 g of water freezes at 272.63 K . Calculate the osmotic pressure of blood at 300 K . (Assume density of blood at 300 K to be 1 g c c^(-1) )

What is the molar mass of a gas whose density is 1.5 g L^(-1) at 27^(@)C and 1 atm pressure ? (Use R = 0.08L atm mol^(-1) K^(-1) )