Home
Class 11
CHEMISTRY
A gas mixture composed of N(2) and O(2) ...

A gas mixture composed of `N_(2) and O_(2)` gases has a density of `1.17g*L^(-1)` at `27^(@)C` and 1 atm pressure. Calculate the mass percents of `N_(2) and O_(2)` in the mixture. Assume that the gas mixture behaves like an ideal gas.

Promotional Banner

Similar Questions

Explore conceptually related problems

The density of a gas at 27^(@)C and 1 bar pressure is "2.56 g L"^(-1) . Calculate the molar mass.

At 127^(0)C and 1 atm pressure, a mixture of a gas contains 0.3 moles of N_(2),0.2 moles of O_(2) ,the volume of the mixture is ( in L )

At 127°C and l atm pressure, a mixture of a gas contains 0.3 mole of N_(2) , 0.2 mole of O_(2) The volume of the mixture is

A mixture of N_(2) and O_(2) at 1 bar pressure contains 80% N_(2) by weight. Calculate the partial pressure of N_(2) in the mixture.

At 127°C and latm pressure, a mixture of a gas contains 0.3 mole of N_(2) , 0.2 mole of O_(2) The volume of the mixture is

The density of gas was found to be 2.92 g L^(-1) at 27° C and 2.0 atm . Calculate the molar mass of the gas.

The density of a gaseous mixture O_(2) and N_(2) is 1.4 g/L at S.T.P. Find out the partial pressure of O_(2) in the mixture.

In a mixture of N_2 and CO_2 gases, the partial pressure of CO_(2) is 1.25 atm. The total pressure of the mixture is 5 atm. The mole fraction of N_(2) in the mixture is