The $rms$ speed of hydrogen molecules at room temperature $(300 \ K)$ will be:

The effect of temperature on Maxwell's speed distribution is correctly shown by

The temperature at which the root mean square velocity of hydrogen molecules equals their escape velocity from the Earth is closest to: [Boltzmann constant $k_B = 1.38 \times 10^{-23} \, J/K$,Avogadro number $N_A = 6.02 \times 10^{23} \, mol^{-1}$,Molar mass of $H_2 = 2 \times 10^{-3} \, kg/mol$,Radius of Earth $R_e = 6.4 \times 10^6 \, m$,Gravitational acceleration $g = 10 \, m/s^2$]

The average speed $\bar{v}$ and $r.m.s.$ speed $v_{rms}$ of the molecules are related as

The relation between root mean square speed $(v_{rms})$ and most probable speed $(v_{p})$ for the molar mass $M$ of oxygen gas molecule at the temperature of $300\, K$ is:

If the r.m.s. speed of a chlorine molecule is $490\,m/s$ at $27^{\circ}C$,the r.m.s. speed of argon molecules at the same temperature will be $......\,m/s$ (Atomic mass of argon $= 39.9\,u$,molecular mass of chlorine $= 70.9\,u$). (in $.7$)