Consider a mixture of gas molecules of type $A,B$ and $C$ having masses, $m_A<m_B<m_C$. The ratio of their root-mean-square speeds at normal temperature and pressure is :

Q. A gas mixture consists of molecules of types $A,B$ and $C$ with masses $m_A>m_B>m_C$. Rank the three types of molecules in decreasing order of

A) Average kinetic energy.

B) rms speeds.

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

Q. The molecules of a given mass of a gas have root mean square speeds of $100$m $s^{-1}$ at $27$ ${}^{o}C$ and $1$ atmospheric pressure. The root mean square speeds of the molecules of the gas at $127$ ${}^{o}C$ and $2$ atmospheric pressure is?

Q. A gas bulb of $1litre$ capacity contains $2.0\times {10}^{21}$ molecules of nitrogen exerting a pressure of $7.57\times {10}^{3}N{m}^{-2}$. Calculate the root mean square speed and temperature of the gas molecules. If the ratio of most probable speed to the root mean square speed is $0.82$, calculate the most probable speed of these molecules at this temperature.

Q. The root mean square speed of molecules of a given mass of a gas at $27°\text{C}$ and $1$atmosphere pressure is $200{\text{ms}}^{-1}$. The root mean square speed of molecules of the gas at $127°\text{C}$ and $2$ atmosphere pressure is $\frac{x}{\sqrt{3}}{\text{ms}}^{-1}$
. The value of $x$ will be .