`0.5 mol` of `H_(2)`, `SO_(2)`, and `CH_(4)` is kept in a container. A hole was made in the container. After `3 hours`, the order of partial pressure in the container will be

Options

A. `p_(SO_(2)) gt p_(CH_(4)) gt pH_(2)`
B. `p_(H_(2)) gt p_(SO_(2)) gt p_(CH_(4))`
C. `p_(CH_(4) gt P_SO_(2) gt P_(H_(2))`
D. `p_(H_(2)) gt p_(CH_(4)) gt p_(SO_(2))`

Answer

A

Explanation

According to Graham's law of diffusion , under identical conditions of `T` and `p` , the rates of diffusion for gaseous substances are inversely proportional to the square roots of their molar masses :
`r prop (1)/(sqrt(M))`
`H_(2)` with the lowest molar mass has the fastest rate of diffusion while `SO_(2)` with the highest molar mass has the slowest rate of diffusion. Hence , the order of partial pressures in the container will be
`p_(SO_(2)) gt p_(CH_(4)) gt p_(H_(2))`