A)A mixture of xenon and
helium gases, at a total pressure of
851 mm Hg, contains 30.4 grams of
xenon and 0.519 grams of
helium. What is the partial pressure of each gas
in the mixture?
PXe = mm Hg
PHe = mm Hg
B)A mixture of helium and argon gases contains helium at a partial pressure of 487 mm Hg and argon at a partial pressure of 471 mm Hg. What is the mole fraction of each gas in the mixture?
XHe =
XAr =
According to Dalton's Law of partial pressure , Partial pressure of gas in mixture = X gas ( P total )
Where X gas is mole fraction of gas.
First calculate no. of moles & mole fraction of each gas.
We know that , No. of moles = Mass / Molar mass
No. of moles of Xe ( n Xe ) = 30.4 g / ( 131.30 g /mol ) = 0.2315 mol
No. of moles of He ( n He ) = 0.519 g / ( 4.00 g / mol ) = 0.1298 mol
Mole fraction of Xe = Moles of Xe / Total moles of gas = n Xe / ( n Xe + n He )
Mole fraction of Xe = 0.2315 / ( 0.2315 + 0.1298 ) = 0.641
Mole Fraction of He = n He / ( n Xe + n He )
Mole fraction of He = 0.1298 / ( 0.2315 + 0.1298 ) = 0.359
Partial pressure of Xe = 0.641 ( 851 mm Hg ) = 545 mm Hg
Partial pressure of He = 0.359 ( 851 mm Hg ) =306 mm Hg
ANSWER : P Xe = 545 mm Hg & P He = 306 mm Hg
PART 2
First calculate total pressure of gas
P total = P He + P A r
Therefore, P total = 487 mm Hg + 471 mm Hg = 958 mm Hg
According to Dalton's Law of partial pressure , Partial pressure of gas in mixture = X gas ( P total )
Where X gas is mole fraction of gas.
Therefore, X gas = Partial pressure of gas / P total
X He = 487 mm Hg / 958 mm Hg = 0.508
X Ar = 471 mm Hg / 958 mm Hg = 0.492
ANSWER : X He = 0.508 & X Ar = 0.492
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