Mean Speed and RMS Speed

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

A real gas follows Boyle's law at :

Discuss the assumptions made for deriving Boyle's law and deviations of a real gas from this law. 

Derive the Boyle's law on the basis of kinetic theory . 

On which of the following factors does the average KE per unit mass of gas molecules depend ? 

(i) Nature of the gas.

 (ii) Absolute temperature.

(iii) Volume.

 What will be irs value at the absolute zero?

Two perfect gases at temperatures ${\mathrm{T}}_1, {\mathrm{T}}_2$ are mixed. There is no loss of energy. Find the temperature of the mixture, if the masses of the molecules are 

${\mathrm{m}}_1\mathrm{and} {\mathrm{m}}_2$ and the number of molecules are ${\mathrm{n}}_1\mathrm{and} {\mathrm{n}}_2$ respectively.

A gas is stored at  $-68°\mathrm{C}$. To what temperature should it be raised so that its average kinetic energy of the molecules is doubled?

The average thermal energy per mole of helium at $27° \mathrm{C}$ is :

Deduce an expression for the kinetic energy of a gas in terms of  its pressure.

Diatomic molecules like hydrogen, have energies due to both translational as well as rotational motion. From the equation $\mathrm{\rho V}=\frac{2}{3}\mathrm{E}$,

$\mathrm{E}$ is :

A molecule of nitrogen has its r m s speed at the surface of the earth at $0°\mathrm{C}$. If it has to go straight up without colliding with other molecules, how high would it rise? The mass of the nitrogen molecule=$4.46\times {10}^{-26 }\mathrm{kg}$ and the Boltzmann's constant ${\mathrm{K}}_{\mathrm{B}}=1.38\times {10}^{\mathrm{\_}23 }\mathrm{J} {\mathrm{molK}}^{-1}$.

Estimate the average thermal energy of a helium atom at (i) room temperature of $27°\mathrm{C}$, (2) at the surface of the sun $\left(6000 \mathrm{K} \right)$ and (iii) in the core of the sun ($10 \mathrm{million} \mathrm{K}$)

Explain the relation of the Kinetic energy of the gas with its temperature.

Deduce an expression of the kinetic energy per gram mol. of a gas.

Explain root mean square velocity of gas molecules and give its expression..

Calculate the rms and mean kinetic energy of one gram of molecules of hydrogen at NTP. (The density of hydrogen at NTP=$0.09 \mathrm{kg}/{\mathrm{m}}^3$)

One mole of an ideal gas is contained in a cube of volume $\mathrm{V}$,as shown in the figure. One face$\mathrm{EFGH}$ is made up of absorbing material,

which absorb all the molecules falling on it.At any given time :

The r.m.s. velocity of hydrogen molecules at NTP is $1.84 {\mathrm{kms}}^{-1}$. Calculate the rms velocity of oxygen molecules at NTP. . The molecular weights of the two gases are $2$ and $32.$

Derive an expression for the pressure of am ideal gas in terms of its r.m.s. velocity.

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