Effusion

A gaseous mixture containing equal mole sof H_(2),O_(2) and He is subjected to series of effusion steps. The composition (by moles) of effused mixture after 4 effusion steps is x:1:y rspectively. Then find the value of ((x)/(y)).

The rate of effusion of an unknown gas (X) through a pinhole is found to be 0.279 times the rate of effusion of hydrogen gas through the same pinhole, if both are at STP. What is the molecular mass of the unknwon gas ?

At 800^(@)C, the following equilibrium is established as F_(2)(g)hArr2F(g) The cojmpositionof equilibrium may be determinded by measuring the rate of effusion of theh kmixture through a pin hole. It is found that at 800^(@)C and 1 atm mixture effuses 1.6 times as fast as SO_(2) effuse under the similar conditions. (At. mass of F = 19 ) what is the value of K_(p) (in atm) ?

The composition of the equilibrium mixture ( Cl_(2) 2Cl ) , which is attained at 1200^(@)C , is determined by measuring the rate of effusion through a pin hole. It is observed that a 1.80 mm Hg pressure, the mixture effuses 1.16 times as fact as krypton effuses under the same conditions. Calculate the fraction of chlorine molecules dissociated into atoms (atomic weight of Kr is 84 ).

A gaseous mixture comprising of equal moles of H_(2)//O_(2)//M (M mass=128) was subjected to series of effusion steps. What will be the number effusion steps required so as to change the composition to: One in which lightest: Heaviest gas is 4096:1 What will be the composition of this mixture (w.r.t all the gases)?