Maxwell's Speed Distribution Law

The ratio amongst most probable velocity, mean velocity and root mean square velocity is given by

At what temperature the root-mean-square speed of nitrogen at $27 °\mathrm{C}$ would be tripled?

The average speed of gas molecules is equal to 

Assertion: Consider a system of gas having N molecules; Instantaneous K.E. of few molecules can be greater than average K.E. of the molecules of the given gas.

Reason: Number of molecules having most probable speed is greater than number of molecules having average speed.

The gas having average speed four times as that of $\mathrm{S}{\mathrm{O}}_2$ (molecular mass 64) at the same temperature, is

Let $\overline{v}$, v_rms and v_p respectively denote the mean speed, the root-mean-square speed, and the most probable speed of the molecules in an ideal monoatomic gas at absolute temperature T. The mass of a molecules is m -

The rms speed of hydrogen is $\sqrt{7}$ times the rms speed of nitrogen. If $T$ is the temperature of the gas, then

An ideal gas is maintained at constant pressure. If the temperature of an ideal gas increases from $100 K to 10000 K$.What affect does it cause on the rms Speed?

Which of the following gases will have least rms speed at a given temperature?

Which of the following statement is wrong about Maxwell's distribution curve?

What happens when the gas becomes hotter?

How can we find the most probable speed of molecules using maxwell's distribution curve for velocities of molecules of a gas?

Area under maxwell distribution represents the number of number of molecules per unit volume.

The speed of sound in hydrogen gas at N.T.P is $1328 \mathrm{m} {\mathrm{s}}^{-1}$ If the density of hydrogen is $\frac{1^{th}}{16}$ of that of air, then the speed (in $\mathrm{m} {\mathrm{s}}^{-1}$ ) of sound in air at N.T.P is (air can be taken as a diatomic gas)

If $m$ represents the mass of each molecule of a gas and $T$ its absolute temperature, then the root mean-square velocity of the gaseous molecule is proportional to

$N (<100)$ molecules of a gas have velocities $1,2,3,...\mathrm{N} \mathrm{km} {\mathrm{s}}^{-1}$ respectively. Then

An ${\mathrm{N}}_2$ molecule is $14$ times heavier than a ${\mathrm{H}}_2$ molecule. At what temperature will the rms speed of ${\mathrm{H}}_2$ molecule be equal to that of ${\mathrm{N}}_2$ molecule at $27°\mathrm{C}$?

The velocity of five particles in $\mathrm{m} {\mathrm{s}}^{-1}$ are $3, 9, 4, \sqrt{15}, 2$. Calculate r.m.s. speed in $\mathrm{m} {\mathrm{s}}^{-1}$.

The root mean square velocity of a perfect gas is

The root mean square velocity of a gas molecule at $27 \mathrm{℃}$ is $1365 \mathrm{m} {\mathrm{s}}^{-1}$. The gas is