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Consider a mixture of gas molecule of types $A, B$ and $C$ having masses $m_{A}\,<\,m_{B}\,<\,m_{C}$ ratio of their root mean square speeds at normal temperature and pressure is :
A closed vessel contains $10 g$ of an ideal gas $X$ at $300 \ K$, which exerts $2$ atm pressure. At the same temperature, $80 g$ of another ideal gas $Y$ is added to it and the pressure becomes $6 atm$. The ratio of root mean square velocities of $X$ and $Y$ at $300 \ K$ is
Two gases-argon (atomic radius $0.07 \;\mathrm{nm}$,atomic weight $40$ ) and xenon (atomic radius $0.1\; \mathrm{nm},$ atomic weight $140$ ) have the same number density and are at the same temperature. The raito of their respective mean free times is closest to
A cylinder of $5$ litre capacity, filled with air at $N.T.P.$ is connected with another evacuated cylinder of $30$ litres of capacity. The resultant air pressure in both the cylinders will be ...... $cm$ of $Hg$
What will be the effect on the root mean square velocity of oxygen molecules if the temperature is doubled and oxygen molecule dissociates into atomic oxygen?
A $25\times10^{-3}\, m^3$ volume cylinder is filled with $1\, mol$ of $O_2$ gas at room temperature $(300\, K)$. The molecular diameter of $O_2$, and its root mean square speed, are found to be $0.3\, nm$ and $200\, m/s$, respectively. What is the average collision rate (per second) for an $O_2$ molecule?