A closed container holds a mixture of `H_(2),SO_(2)` and `CH_(4)` gases, each with an amount off 0.5 mol. If these gases effuse through a fine orifice in the container, arrange them in the increasing order of their partial pressure once the effusion begins.

Explanation

According to the Graham's law of diffusion, at constant temperature and pressure, the rate of effusion of a gas is inversely proportional to the square root off its molar mass, i.e.,
`r prop(1)/(sqrt(M))`.
The increasing order of molar masses of the given gases is `M_(H_(2)) lt M_(CH_(4)) lt M_(SO_(2))`. so, the order of the rate of effusion of these gases at a particular temperature and pressure will be `r_(H_(2)) gt r_(CH_(4)) gt M_(SO_(2))`. so, the order of the rate of effusion of these gases at a particular temperature and pressure will be `r_(H_(2)) gt r_(CH_(4)) gt r_(SO_(2))`. once effusion begins, the order of their number of moles will be `n_(H_(2)) lt n_(CH_(4)) lt n_(SO_(4))`. therefore, the order of their partial presures will be `p_(H_(2)) lt p_(CH_(4)) lt p_(SO_(2))`.