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In a vessel an equilibrium mixture at 300k contained N2O2 and NO2 gases at partial pressures 100 atm and 10 atm respectively . the volume of the container is doubled at the same temperature. then the partial pressures of N2O2 and NO2 gases are (in atm )
Total Pressure = sum of individual partial pressures of gases.Pt = 100 + 10 = > 110 atm.From the ideal gas eqn.PtV = nRT110V = (n1+n2)RT.........(1)Pt(2V) = (n1+n2)RT..............(2)Dividing the eqns. we get,Pt = 55 atm. Now for both gases individually,100V = n1RT and 10V = n2RTfrom these two relations,n1 = 10n2.................(3)andafter doubling the volume,P1(2V) = n1RTandP2(2V) = n2RTfrom these two relations,P1/P2 = n1/n2 = 10orP1 = 10P2Now total pressure calculated after doubling the volume,Pt => 55 = P1 + P2 or10P2 + P2 = 5511P2 = 55P2 = 5 atmand P1 = 55 - 5 => 50 atm.
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