Diffusion of Gas

Two gases A and B having the same volume diffuse through a porous partition in 20 and 10 seconds respectively. The molecular mass of A is 49 u. Molecular mass of B will be:

From a heated mixture of nitrogen, oxygen and carbon, two compounds (out of the many obtained) are isolated. The rates of diffusion of the two isolated compounds are almost identical. The two compounds are

If two molecules of $\mathrm{A}$ and $\mathrm{B}$ having mass $100 \mathrm{Kg}$ and $64 \mathrm{Kg}$ and rate of diffusion of $\mathrm{A}$ is $12\times {10}^{-3}$, then rate of diffusion of $\mathrm{B}$ will be

From a certain apparatus, the diffusion rate of hydrogen has an average value of $28.7 \mathrm{c}{\mathrm{m}}^3\mathrm{ }{\mathrm{s}}^{-1}$. The diffusion of another gas under the same conditions is measured to have an average rate of $7.2 {\mathrm{cm}}^3{\mathrm{s}}^{-1}$. Identify the gas.

A mixture of ${\mathrm{H}}_2$ and ${\mathrm{O}}_2$ taken in a bulb in $2 : 1$ mole ratio is allowed to diffuse through a fine hole. The composition of the gases (mole ratio) coming out initially will be:

From a certain apparatus, the diffusion rate of hydrogen has an average value of $28.7 \mathrm{c}{\mathrm{m}}^3\mathrm{ }{\mathrm{s}}^{-1}$. The diffusion of another gas under the same conditions is measured to have an average rate of $7.2 {\mathrm{cm}}^3{\mathrm{s}}^{-1}$. Identify the gas.(Oxygen/Nitrogen)

The degree of dissociation $\left(\mathrm{\alpha }\right)$ of the reaction ${{\mathrm{A}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{A}}_{\left(\mathrm{g}\right)}$  in terms of rate of diffusion $\left({\mathrm{r}}_{mix}\right)$ of equilibrium mixture and that of a reference gas $\mathrm{C}$ is given by: 

where $\mathrm{M}$ stands for the respective molar masses.

In $5 \mathrm{s}$, the volume $\mathrm{X}$of ${\mathrm{H}}_2$ gas effuses through a hole in a container. The time taken for the effusion of the same volume of the specified gas under identical conditions is

$50 \mathrm{mL}$ of each gas $\mathrm{A}$ and of gas $\mathrm{B}$ takes $150$ and $200$ seconds respectively for effusing through a pin hole under the similar conditions. If molecular mass of gas $\mathrm{A}$ is $36$, the molecular mass of gas $\mathrm{B}$ will be :

Which pair of the gaseous species diffuse through a small jet with the same rate of diffusion at same $\mathrm{P}$ and $\mathrm{T}$ :-

What is the ratio of diffusion rate of oxygen to hydrogen?

A certain gas takes three times as long to effuse out as helium. Its molecular mass will be

Under identical experimental conditions, which one of the following pairs of gases will be most easy to separate by diffusion process?

If the four tubes of a car are failed to the same pressure with ${\mathrm{N}}_2, {\mathrm{O}}_2, {\mathrm{H}}_2 \mathrm{and} \mathrm{Ne}$ separately then which one will be filled first?

The densities of hydrogen and oxygen are 0.09 and 1.44 g L^–1. If the rate of diffusion of hydrogen is 1, then that of oxygen in the same units will be:

$5\mathrm{mL}$ of $He$ gas diffuses out in one second from a hole. Find the volume of ${\mathrm{SO}}_2$ that will diffuse out from the same hole under identical conditions in two seconds.

Gas $\text{'}\mathrm{A}\text{'}$ has $1/2$ rate of diffusion than gas ${}^{\text{'}}\mathrm{B}^{\text{'}}.$ If molecular mass of gas $\mathrm{A}$ is $16 \mathrm{g}$, then calculate molecular mass of gas $\text{'}\mathrm{B}\text{'}$:

The rate of effusion of helium gas at a pressure of $1000 \mathrm{torr}$ is $10 \mathrm{torr} {\min }^{-1}.$ What will be the rate of effusion of hydrogen gas at a pressure of $2000 \mathrm{torr}$, at the same temperature?

The ratio of rates of diffusion of ${\mathrm{SO}}_2, {\mathrm{O}}_2$ and ${\mathrm{CH}}_4$ under identical conditions is:

The rate of diffusion of gas having molecular weight just double that of nitrogen gas is $56 \mathrm{ml} {\mathrm{s}}^{-1}$. The rate of diffusion of nitrogen will be: