Question

A gaseous mixture contains 414.0 Torr of H2(g), 373.5 Torr of N2(g), and 90.1 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases.

X_{h2 = ?}

X_{n2 = ?}

X_{ar = ?}

Answer 1

total pressure(Ptotal) = 414+373.5+90.1 = 877.6 torr

partial pressure of H2(pH2) = XH2*pTotal

                414 = x*877.6

   XH2 = molfraction of H2 = x = 0.472

partial pressure of N2(pN2) = XN2*pTotal

                373.5= x*877.6

   XN2 = molfraction of N2 = x = 0.4256

partial pressure of Ar(pAr) = XAr*pTotal

                90.1 = x*877.6

   XAr = molfraction of Ar = x = 0.103