Four molecules of a gas have speeds $1, 2, 3$ and $4 \ km/s$. The value of root mean square speed of the gas molecules is

The $rms$ speed of oxygen at $27^{\circ}C$ will be .... $ms^{-1}$.

The temperature at which the root mean square velocity of a molecule will be doubled than its value at $100^{\circ}C$ is:

At temperature $T$,$N$ molecules of gas $A$ each having mass $m$ and at the same temperature $2N$ molecules of gas $B$ each having mass $2m$ are filled in a container. The mean square velocity of molecules of gas $B$ is $v^2$ and the mean square of the $x$-component of velocity of molecules of gas $A$ is $w^2$. The ratio of $w^2/v^2$ is:

The root mean square velocity of molecules of a gas is $200 \,m/s$. What will be the root mean square velocity of the molecules, if the molecular weight is doubled and the absolute temperature is halved?

The temperature of an ideal gas is increased from $27^{\circ} C$ to $927^{\circ} C$. The r.m.s. speed of its molecules becomes