A mixture of gases contains` H_(2)` and `O_(2)` gases in the ratio of 1:4 (w//w). What is the molar ratio of the two gases in the mixture?
1 4:1
2 16:1
3 2:1
4 1:4

A mixture contains N_(2)O_(4) and NO_(2) in the ratio 2:1 by volume. Calculate the vapour density of the mixture?

A gaseous mixture containing He, CH_(4) and SO_(2) in 1:2:3 mole ratio, calculate the molar ratio of gases effusing out initially.

The densities of two gases are in the ratio of 1 : 16 . The ratio of their rates of diffusion is

The densities of two gases are in the ratio of 1:16. The ratio of their rates of diffusion is

The vapour densities of two gases are in the ratio of 1 : 3 . Their molecular masses are in the ratio of : -

The rates of diffusion of two gases A and B are in the the ratio 1:4 A mixture contains these gases A and B in the ratio 2:3 The ratio of mole fraction of the gases A and B in the mixture is (assume that P_(A) =P_(B)) .

If the ratio of molar masses of two gases A and B is 1 : 4. What is the ratio of the average speeds ?

Densities of two gases are in the ratio 1: 2 and their temperatures are in the ratio 2:1 , then the ratio of their respective pressure is

If the ration of the masses of SO_(3) and O_(2) gases confined in a vessel is 1 : 1 , then the ratio of their partial pressure would be

If the ration of the masses of SO_(3) and O_(2) gases confined in a vessel is 1 : 1 , then the ratio of their partial pressure would be