If the temperature of gas molecules is raised from $127^{\circ} C$ to $527^{\circ} C$,the ratio of the r.m.s. speed of the molecules is respectively:

The $rms$ speeds of the molecules of Hydrogen,Oxygen,and Carbon dioxide at the same temperature are $V_{H}$,$V_{O}$,and $V_{C}$ respectively. Then:

The $rms$ speed of $n$ molecules in a gas having speeds $\upsilon_1, \upsilon_2, \upsilon_3, \dots, \upsilon_n$ is equal to:

The molecules of a given mass of a gas have root mean square speeds of $100 \ m/s$ at $27^{\circ} \ C$ and $1.00 \ \text{atm}$ pressure. What will be the root mean square speeds of the molecules of the gas at $127^{\circ} \ C$ and $2.0 \ \text{atm}$ pressure?

At a given temperature,the root mean square velocities of oxygen and hydrogen molecules are in the ratio:

The temperature of an ideal gas is increased from $100 \ K$ to $400 \ K$. If '$x$' is the root mean square velocity of its molecules at $100 \ K$,what is the new root mean square velocity?