The root mean square of gas molecules at 25 K and 1.5 bar is ${\text{100 m s}}^{-1}$. If the temperature is raised to 100 K and the pressure to 6.0 bar, the root mean square speed becomes

The root mean square speed of gas molecules

The root mean square velocity of a gas molecule at 100 K and 0.5 atm pressure is $106.4m{s}^{-1}$. If the temperature is rasied to 400 K and the pressure is raised to 2 atm, then root mean square velocity becomes

The root mean square velocity of a gas molecule at 100K and 0.5 atm pressure is 106.4$m{s}^{-1}$. If the temperature is raised to 400K and the pressure is raised to 2 atm, the root mean square velocity becomes:

The root mean square velocity of a gas molecule at any temperature T K of a gas molecule of molecular weight M is

The root mean square speed of the molecules of a gas is

The root mean square speed of gas molecules at a temperature $27K$ and pressure 1.5 bar is $1\times {10}^{4}cm/\sec$ If both temperature and pressure are raised three times calculate the new rms speed of gas molecules .

The root mean square speed of the molecules of a diatomic gas is v. When the temperature is doubled, the molecules dissociates into two atoms. The new root mean square speed of the atom is

The root mean spuare (rms) speed of hydrogen molecules at a certain temperature is 300m/s. If the temperature is doubled and hydrogen gas dissociates into atomic hydrogen the rms speed will become

The root mean square velocity of a gas molecule of mass m at a given temperature is proportional to

The root mean square velocity of a gas molecule of mass m at a given temperature is proportional to