Question

A mixture of hydrogen and helium gases, at a total pressure of 942 mm Hg, contains 0.365 grams of hydrogen and 0.421 grams of helium. What is the partial pressure of each gas in the mixture? PH Рне mm Hg mm Hg

Answer 1

solution 1 Moss of lydroge w=0.365 g Mass of heliuw -0.421 g ند moles of lydrogen weight in grow Molar maps 0.365 g = 0-362 mol 1'008 g/mol hole of helium 0.4219 = 0.105 mol 4.00 g/mol Total number of moles=10.362 +0.105 mol =0.467 mol Mole fraction Keember of moles of component total number of holes Xuydrogen 0.362 mot = 0.775 0.467 hot y helium 1 -0.715 = 0.225 At equilibrier partial Pressure of component is calculated by Daltow's low at partial Pressure PHz = x, Ptotal = 0 775 942 mm multg = 730.05 mmHg Pine = X₂ Ptatal 0.225 x 942 hm Hg = 211.95 mm Hg

0.2 AS :- Partial Pressure of nitrogen = Partial Pressure of Argow 299 multa q91 mmHg Solution Phase Pressure in Ptotal - Pit P2 لیل Ptotal 379 muilla +291 mmity .670 mmHg At equilibriuw partial pressure of component is calculated by Pi = yl total colore = mole fractions as 42= mole fractical Cowloonent 2 a^ mole fractionow of nitrogen Y Partial Pressure 379 multa oted Pressure 670 hore ng 81 Pre = 12 total = 0.565 mole freefrow of Argon 291 mullg nuity 670 mul = 0.434 Toso I hole fraction of nitroge = 0.565 mole fraction of Argou 20 434