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 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 container of volume V = 16.6 litre contains a mixture of hydrogen and helium at a temperature of 300 K. The pressure in the container is 6 x× 10^(5) Pa and mass of the mixture is 10 g. Let f_(1) " and " f_(2) be the number of collisions made by the hydrogen and helium molecules with unit area of the container wall in unit time. Calculate the ratio (f_(1))/(f_(2)) . [R = 8.3 "J mol"^(–1) K^(–1)] .

A closed container of volume 0.02m^(3) contains a mixture of neon and argon gases at a temperature 27^(@)C and pressure 1 xx 10^(5) Nm ^(-1) The total mass of and argon are 20 and 40 respectively find the masses of individual gases in the container assuming then to be ideal .