Kinetic Molecular Theory of Gases

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

Which of the following is not true in case of an ideal gas ?

Write the effect of the molar mass on Maxwell-Boltzmann's distribution curve of molecular speeds.

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.

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)

Among the following, the plot that shows the correct marking of most probable velocity $\left({\mathrm{V}}_{\mathrm{MP}}\right),$ average velocity $\left(\overline{\mathrm{V}}\right),$ and root mean square velocity $\left({\mathrm{V}}_{\mathrm{RMS}}\right)$ is :

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

Gases consists of large number of identical particles (atoms or molecules ) that are so small and so far apart on the average that the actual volume of the molecules is negligible in comparison to the empty space between them. This assumption explains the 

The $\mathrm{RMS}$ speed of ${\mathrm{N}}_2$ in a gas is $\mathrm{u}.$ If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms, the new $\mathrm{RMS}$ speed of the atoms will be _____

A bottle contains $1.0 \mathrm{mol} \mathrm{He} \left(\mathrm{g}\right)$ and a second bottle contains $1.0 \mathrm{mol} \mathrm{Ar} \left(\mathrm{g}\right)$ at the same temperature. At this temperature, the root mean square speed of $\mathrm{He}$ is $1477 \mathrm{m} {\mathrm{s}}^{-1}$ and that of $\mathrm{Ar}$ is $467 {\mathrm{ms}}^{-1}$. What is the ratio of the number of $\mathrm{He}$ atoms, in the first bottle to the number of $\mathrm{Ar}$ atoms, in the second bottle having these speeds? Assume that both gases behave ideally?

The ratio of most probable velocity to the average velocity is

By what factor does the average velocity of a gaseous molecule increase when the absolute temperature is doubled ?

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?

According to graham’s Law at a given temperature, the ratio of the rates of diffusion ${\mathrm{r}}_{\mathrm{A}}/{\mathrm{r}}_{\mathrm{B}}$ of gases A and B is given by

Name the term used for mixing of different gases by random molecular motion and frequent collision. (diffusion/osmosis)

A mixture containing $1.12$ litres of ${\mathrm{H}}_2$ and $1.12$ litres of ${\mathrm{D}}_2$ at $\mathrm{NTP}$ is taken inside a bulb connected to another bulb by a stopcock with a small opening. The second bulb is fully evacuated, the stopcock opened for a certain time and then closed. The first bulb is now found to contain $0.05 \mathrm{g}$ ${\mathrm{H}}_2$. Determine the percentage composition by weight of the gases in the second bulb.