How does the $rms$ velocity of an ideal gas vary with density at constant pressure?

At a temperature of $27 \, ^\circ C$,the $rms$ speed of a gas is $1930 \, m/s$. The gas is:

The temperature of an ideal gas is increased from $200 \ K$ to $800 \ K$. If the r.m.s. speed of the gas at $200 \ K$ is $v_0$,then the r.m.s. speed of the gas at $800 \ K$ will be:

Five gas molecules chosen at random are found to have speeds of $500, 600, 700, 800$ and $900 \ m/s$. Which of the following statements is correct?

The root mean square (rms) velocity of an ideal gas at temperature $T$ is $v$. If the temperature is increased to $4 T$, the rms velocity of the gas is

At what temperature is the root mean square (rms) speed of Neon gas atoms equal to the rms speed of Helium gas atoms at $-33^{\circ} C$ (in $K$)? (Atomic mass of $Ne = 20.2 \ u$ and that of $He = 4.0 \ u$)