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A gaseous mixture contains 413.0 Torr of H2(g), 391.5 Torr of N2(g), and 65.7 Torr of...

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Chemistry

A gaseous mixture contains 413.0 Torr of H2(g), 391.5 Torr ofN2(g), and 65.7 Torr of Ar(g). Calculate the mole fraction, X, ofeach of these gases.

Answer & Explanation Solved by verified expert
4.0 Ratings (764 Votes)

PH2    =413 Torr

PN2    = 391.5 Torr

PAr     = 65.7 Torr

Total pressure = PH2 + PN2 + PAr

                         = 413+391.5 +65.7 =870.2 Torr

partial pressure   = mole fraction of gas* total pressure

PH2                   = XH2 * PT

413                    = XH2 *870.2

XH2                     = 413/870.2    = 0.475

PN2                   = XN2 * PT

391.5                 = XN2 *870.2

XN2                    = 391.5/870.2   = 0.45

PAr                   = XAr * PT

65.7                 = XAr *870.2

XAr                   = 65.7/870.2   = 0.0755
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