A flask contains argon and chlorine in the ratio of \(2:1\) by mass. The temperature of the mixture is \(27~^\circ\mathrm{C}\). The ratio of average kinetic energy per molecule of the molecules of the two gases is: 
(Atomic mass of argon = \(39.9~\text{u}\); Molecular mass of chlorine = \(70.9~\text{u}\))
1. \(1:2\)
2. \(2:1\)
3. \(1:1\)
4. \(1:2\)

A flask contains argon and chlorine in the ratio of \(2:1\) by mass. The temperature of the mixture is \(27^{\circ}~\mathrm{C}\). The ratio of root mean square speed \(v_{rms}\) of the molecules of the two gases is: (Atomic mass of argon = \(39.9~\text{u},\) Molecular mass of chlorine = \(70.9~\text{u}\))
1. \(2.33\)
2. \(1.33\)
3. \(0.5\)
4. \(2\)

Uranium has two isotopes of masses \(235 \) and \(238\) units. If both are present in Uranium hexafluoride gas, which would have the larger average speed?
1. \(^{235} \mathrm{U} \mathrm{F}_{6}\)
2. \({}^{238} \mathrm{U} \mathrm{F}_{6}\)
3. Both will have the same average speed.
4. Data insufficient