Six molecules of an ideal gas have velocities $1, 3, 5, 5, 6$ and $5 \,m/s$ respectively. At any given temperature, if $\overline{V}$ and $V_{rms}$ represent average and rms speed of the molecules, then

The r.m.s. speed of hydrogen at $S.T.P.$ is $u \text{ m/s}$. If the gas is heated at constant pressure till its volume becomes three times, the final temperature of the gas and the r.m.s. speed are respectively:

$V_{rms}$ denotes the root mean square speed,$\bar{V}$ the average speed,and $V_m$ the most probable speed of gas molecules. Which of the following is the correct relationship?

The rms speed of an oxygen molecule at a certain temperature is $600 \,ms^{-1}$. If the temperature is doubled and the oxygen molecule dissociates into atomic oxygen atoms,the new rms speed is (in $\,ms^{-1}$)

The speeds of $5$ gas molecules are $2, 3, 4, 5,$ and $6$ units respectively. What is the $rms$ speed of these molecules?

$N$ molecules each of mass $m$ of gas $A$ and $2N$ molecules each of mass $2m$ of gas $B$ are contained in a vessel which is maintained at temperature $T$. The mean square velocity of the molecules of gas $B$ is denoted by $V_2^2$ and the mean square of the $X$-component velocity of the molecules of gas $A$ is denoted by $V_1^2$, then $\frac{V_1}{V_2}$ is