Two containers A and B have the same volume. Container 'A' contains 5 mole of oxygen gas. Container 'B' contains 3 moles of He gas and 2 mole of $C H_{4}$ gas. Both the containers are separately kept in vaccum at the same temperature. Both the containers have very small orifices of the same area through which the gases leak out. The rate of diffusion of $O_{2}$ is how many times the rate of diffusion of He and $C H_{4}$ mixture.

Q. Find the number of diffusion steps required to separated the isotopic mixture initially containing some amount of

H_{2}

gas and 1 mol of

D_{2}

gas in a container of 3 lit capacity maintained at 24.6 atm and

27^{\circ}

to the final mass ratio

(\frac{W_{D_{2}}}{W_{H_{2}}})

equal to

\frac{1}{4} .

Q. From a certain apparatus, the diffusion rate of hydrogen has an average value of 28.7 cm³ s¯¹. The diffusion of another gas under the same conditions is measured to have an average rate of 7.2 cm³ s¯¹. Identify the gas. [Hint : Use Graham’s law of diffusion: R₁/R₂ = ( M₂ /M₁ )1/2, where R₁, R₂ are diffusion rates of gases 1 and 2, and M₁ and M₂ their respective molecular masses. The law is a simple consequence of kinetic theory.]

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Assume that you have a sample of a gas containing H2, HD and D2 that you want to separate into pure components (H= 1H and D= 2H). What are the relative rates of diffusion of the three gases according to Graham’s law?

Assume that you have a sample of a gas containing $H_{2}, H D$ and $D_{2}$ that you want to separate into pure components $(H =^{1} H and D =^{2} H)$ . What are the relative rates of diffusion of the three gases according to Graham’s law?