A vessel of volume `20 L` contains a mixture o hydrogen and helium at temperature of `27^(@)C` and pressure `2.0 atm` The mass of the mixture is `5 g`. Assuming the gases to be ideal, the ratio of the mass of hydrogen to heat of helium in the given mixture will be

A vessel of volume V = 20 1 contains a mixture of hydrogen and helium at a temperature t = 20 ^@C and pressure p = 2.0 atm . The mass of the mixture is equal is equal to m = 5.0 g . Find the ratio of the mass of hydrogen to that of helium in the given mixture.

A vessel of volume 0.02m^3 contains a mixture of hydrogen and helium at 20^@C and 2 atmospheric pressure. The mass of mixture is 5 gms. Find the ratio of mass of hydrogen to that of helium in the mixture.

A vessel of volume 2 xx 10^(-2) m^(3) contains a mixture of hydrogen and helium at 47^(@)C temperature and 4.15 xx 10^(5) N//m^(2) Pressure. The mass of the mixture is 10^(-2) kg . Calculate the masses of hydrogen and helium in the given mixture.

A vessel of volume 2 xx 10^(-2) m^(3) contains a mixture of hydrogen at 47^(@)C temperature and 4.15 xx 10^(5) N//m^(2) Pressure. The mass of the mixture is 10^(-2) kg . Calculate the masses of hydrogen and helium in the given mixture.

A vessel of volume 2 xx 10^(-2) m^(3) contains a mixture of hydrogen at 47^(@)C temperature and 4.15 xx 10^(5) N//m^(2) Pressure. The mass of the mixture is 10^(-2) kg . Calculate the masses of hydrogen and helium in the given mixture.

A closed container of volume 0.02 m^3 contains a mixture of neon and argon gases at a temperature of 27^@C and pressure of 1 times 10^5 N.m^-2 The total mass of the mixture is 28 g. IF the molar masses of neon and argon are20 and 40 g//mol respectively . find the masses of the individual gases in the container assuming then to be ideal. [R=8.314 J.mol^-1.K^-1 ]

A vessel of volume 4 litres contains a mixture of 8g of O_(2), 14g of N_(2) and 22 g of CO_(2) at 27^(0)C . The pressure exerted by the mixture is