A vessel contains equal masses of `CH_(4) and H_(2)` gas at `25^(@)C`. What part of the total pressure inside the vessel is equal to the partial pressure of `H_(2)` gas?

Explanation

`W_(CH_(4))=W_(H_(2))=W,`
`therefore n_(CH_(4)) =(W)/(16)mol and n_(H_(2)) =(W)/(2)` mol
total mol, `n=((W)/(16)+(W)/(2)) mol=(9W)/(16)` mol
`P=(nRT)/(V)=(9W)/(16V)RT` [V=total volume, P=Total pressure]
`p_(H_(2))=(W)/(2)xx(RT)/(V)" "therefore p_(H_(2)) =(16)/(9)xx(P)/(2)=(8)/(9)P`