Respuesta :
Answer: From the given gases, the greatest rate of effusion is of [tex]CH_4[/tex]
Explanation:
Rate of effusion of a gas is determined by a law known as Graham's Law.
This law states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows:
[tex]\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}[/tex]
It is visible that molar mass is inversely related to rate of effusion. So, the gas having lowest molar mass will have the highest rate of effusion.
For the given gases:
Molar mass of [tex]NH_3=17g/mol[/tex]
Molar mass of [tex]HCl=36.5g/mol[/tex]
Molar mass of [tex]CH_4=16g/mol[/tex]
Molar mass of [tex]Ar=40g/mol[/tex]
Molar mass of [tex]HBr=81g/mol[/tex]
The molar mass of methane gas is the lowest. Thus, it will have the greatest rate of effusion.
Hence, the greatest rate of effusion is of [tex]CH_4[/tex]
