Question

A gaseous mixture contains 418.0 Torr of H2(g), 371.7 Torr of N2(g), and 88.9 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases.

Answer 1

A gaseous mixture contains 418.0 Torr of H2(g), 371.7 Torr of N2(g), and 88.9 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases.

Solution

Let P1 = partial pressure gas
X1 = mole fraction of gas
and Pt = total pressure

P1 = (X1)(Pt)
X1 = P1/Pt

This is derived from
equation of partial pressure gas over total pressure
P = nRT/V
P1 = n1RT/V over Pt = ntRT/V = P1/Pt = n1/nt
Therefore ratio of partial pressure gas/total pressure = mole fraction individual gas
Total pressure: 418.0 + 371.7 + 88.9 = 878.6 torr
X H2 = 418/878.6 = 0.475
X N2 = 371.7/878.6 = 0.423
X Ar = 88.9/878.6 = 0.010

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