Gaseous StateEasy
Question
A sample of gaseous mixture in the beaker contains 6.08 × 1020 molecules of N2, 0.76 × 1020 molecules of O2, and 0.50 × 1020 molecules of CO2. The total pressure is 734 mm of Hg. The partial pressure of O2 would be
Options
A.760.0 mm of Hg
B.76.0 mm of Hg
C.7.6 mm of Hg
D.0.76 mm of Hg
Solution
pO2 = PTotal × χO2 (mole fraction of O2)
χO2 =
χO2 =
pO2 = PTotal × χO2 = 734 ×
= 76.0 mm of Hg.
χO2 =
χO2 =
pO2 = PTotal × χO2 = 734 ×
= 76.0 mm of Hg.
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