$V_{rms}$ 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?

At what temperature (in $K$) is the $rms$ velocity of a hydrogen molecule equal to that of an oxygen molecule at $47^o \ C$?

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

Let $A$ and $B$ be two gases and given: $\frac{T_A}{M_A} = 4 \cdot \frac{T_B}{M_B}$,where $T$ is the temperature and $M$ is the molecular mass. If $C_A$ and $C_B$ are the $r.m.s.$ speeds,then the ratio $\frac{C_A}{C_B}$ will be equal to:

At a given temperature,the $r.m.s.$ velocity of molecules of a gas is

$A$ flask contains argon and chlorine in the ratio of $2:1$ by mass. The temperature of the mixture is $27^{\circ}\text{C}$. The ratio of root mean square speed of the molecules of the two gases $\left(\frac{v_{\text{rms}}^{\text{Ar}}}{v_{\text{rms}}^{\text{Cl}}}\right)$ is : (Atomic mass of argon $= 40.0 \text{u}$ and molecular mass of chlorine $= 70.0 \text{u}$)