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 = \(39.9\) u; Molecular mass of chlorine = \(70.9\) 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?

Uranium has two isotopes of masses 235 and 238 units. If both are present in Uranium hexafluoride gas. If the atomic mass of fluorine is 19 units, what is the percentage difference in speeds of isotopes of Uranium at any temperature?

1.  0.43%

2.  0.34%

3.  0.55%

4.  Data insufficient