Question

Of the following gases, ________ will have the greatest rate of effusion at a given temperature. Of the following gases, ________ will have the greatest rate of effusion at a given temperature. NH3 HCl CH4 Ar HBr

Answer 1

CH4

CH4

Step-by-step explanation:

Answer 2

Answer: From the given gases, the greatest rate of effusion is of
`CH_4`

Step-by-step 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:

`\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}`

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
`NH_3=17g/mol`

Molar mass of
`HCl=36.5g/mol`

Molar mass of
`CH_4=16g/mol`

Molar mass of
`Ar=40g/mol`

Molar mass of
`HBr=81g/mol`

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
`CH_4`