For a gas at room temperature of $27^{\circ}C$,the value of $\nu_{rms}$ is $1930 \, m/s$. The gas is.......... $(R = 8.3 \, J/mol \cdot K)$.

An $HCl$ molecule has rotational,translational,and vibrational motions. If the $rms$ velocity of $HCl$ molecules in its gaseous phase is $\bar{v}$,$m$ is its mass,and $k_B$ is the Boltzmann constant,then its temperature will be:

Consider an ideal gas in a closed container at $300 \ K$. The container is then heated so that the average velocity of particles of the gas increases by a factor of $4$. What would be the final temperature (in $^{\circ} C$)?

The temperature at which the rms speed of molecules in hydrogen gas will be double of its initial value at $27^{\circ} C$ is (in $^{\circ} C$)

Derive the equation of $v_{rms}$ in terms of the mass of a molecule.

The rms speed of an oxygen molecule at a certain absolute temperature is $v$. If the absolute temperature is doubled and the oxygen molecules dissociate into atomic oxygen,then the rms speed would be