How many times greater is the rate of effusion of molecular fluorine than that of molecular bromine at the same temperature and pressure?

According to Graham's law the rates of effusion of two gases are inversely proportional to the square roots of their molar masses at the same temperature and pressure: Effusion is used to describe the passage of a gas through a tiny office into an evacuated chamber.

Therefore;, R1/R2 = √mm2/√mm1

The molecular mass of fluorine is 38 g and that of 160 g

Therefore; = √ (160/38)

= √ 4.211

= 2.051

Hence; the rate of effusion of molecular fluorine is 2.051 times than that of molecular bromine at the same temperature and pressure.