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P tot = 0.1065 atm
The mole fraction of oxygen in the mixture : 0.709
Given
10 L flask
1.013 g O₂
572 g CO₂
T = 18 °C = 291 K
Required
P O₂ and P CO₂
Solution
Dalton Law's of partila pressure
P tot = P₁ + P₂ + ..Pₙ
From ideal gas Law :
[tex]\tt P_{O_2}=\dfrac{\dfrac{1.013}{32}\times 0.082\times 291 }{10}\\\\P_{O_2}=0.0755~atm[/tex]
[tex]\tt P_{CO_2}=\dfrac{\dfrac{0.572}{44}\times 0.082\times 291}{10}\\\\P_{CO_2}=0.031~atm[/tex]
P tot = P O₂ + P CO₂
P tot = 0.0755 + 0.031
P tot = 0.1065 atm
The mole fraction of O₂ :
[tex]\tt P_{O_2}=X_{O_2}\times P_{tot}\\\\X_{O_2}=\dfrac{P_{O_2}}{P_{tot}}\\\\X_{O_2}=\dfrac{0.0755~atm}{0.1065~atm}\\\\X_{O_2}=0.709[/tex]