Effusion of gasses problem... Please help whith this problem...And also explain the reason...

The relative molecular mass (Mr  ) of the gas determines the rate of diffusion of the gases from a region of higher concentration to a region of lower concentration. The smaller the Mr of the gas, the greater the rate of diffusion (movement of gas molecules).

 

Since hydrogen gas has a smaller Mr than carbon dioxide gas, more hydrogen gas diffuse out of the balloon than carbon dioxide gas into the balloon per unit time. Hence, this balloon will shrink.

 

M r of N2O = 44 (Balloon B) Since nitrous oxide gas has a greater Mr than carbon dioxide gas, more carbon dioxide gas diffuse into the balloon than nitrous oxide gas out of the balloon per unit time. Hence, this balloon will inflate

 

Mr of CO= 28 (Balloon C) This balloon will shrink (same logic as \ceH2 \ce H 2 ).

 

Mr of CO2 = 40 (Balloon D) Since the balloon and the tank both contains CO2 (same Mr of gases), there is no net diffusion of gases in/out of the balloon, thus the balloon will not inflate/shrink (theoretically). ​