Given that the temperature of Helium gas is −20 °C, atomic mass of argon is 39.9 u and of helium is 4.0 u.
Let v He be the root mean square velocities of helium, then
v Ar = 3R T Ar M Ar (1)
Here, R is the universal gas constant, T Ar is the temperature of argon gas and M Ar is the atomic mass of argon.
Let v He be the root mean square velocities of Helium, then
v He = 3R T He M He (2)
Here, T He is the temperature of helium gas and M He is the atomic mass of helium.
The root mean square velocity of both the gases is equal, hence
v Ar = v He 3R T Ar M Ar = 3R T He M He T Ar M Ar = T He M He T Ar M Ar = T He M He T Ar = T He M He × M Ar
Substitute the values in the above equation.
T Ar = ( 273+( −20 ) ) 4 ×39.9 = 253 4 ×39.9 =2523.67 K
Hence, at 2523.67 K temperature, the root mean square speed of an atom of argon gas cylinder is equal to that of helium gas atom at −20 °C.