EXERCISE

There is a mixture of hydrogen and oxygen in a vessel. The rms velocity of oxygen molecules is

The wall of a gas container experiences a pressure because

A vessel of volume $5$ litre contains ${10}^{26}$ molecules of a gas. Each molecule has a mass $2.4\times {10}^{-25} \mathrm{g}$. The rms velocity is $3.5\times {10}^4 \mathrm{cm}{ \mathrm{s}}^{-1}$. The pressure approximately is equal to

The kinetic energy per gram molecule of helium gas at $27°\mathrm{C}$ is given by [Given, $\mathrm{R}=8.3\times {10}^7\mathrm{erg} {\mathrm{mole}}^{-1}{ \mathrm{K}}^{-1}$]

If $k$ be the Boltzmann constant and $T$ to the temperature, then the average kinetic energy of each molecule of a gas will be

The pressure for ideal gas is $P$ and the average energy per unit volume is $E$. The relation between $E$ and $P$ is,

The ratio of the most probable velocity $\left(c_{\mathit{m}}\right)$ and $\mathrm{rms}$ velocity $\left(c_{\mathrm{rms}}\right)$ of the molecules of a given gas at a given temperature is

The $\mathrm{rms}$ speed of an ideal gas is $c$. The volume of the gas is doubled keeping its temperature unchanged. The $\mathrm{rms}$ speed will now be