According to Dalton\'s law of partial pressures Total pressure P t = P N2 + P He
ID: 700327 • Letter: A
Question
According to Dalton's law of partial pressures
Total pressure Pt = PN2 + PHe
Where PN2 = partial pressure of N2, PHe = partial pressure of He
There is a relation connecting partial pressure , total pressure and mole fraction.
PN2 = xN2 Pt
Where xN2 is molefraction of N2.
PHe = xHe Pt
Where xHe is molefraction of He.
PHe = xHe Pt
xHe = no.of moles of He/(total no.of moles)
no.of moles of He = mass in grams/molar mass = 18.4 g/4 g/mol = 4.6 mol
no.of moles of N2 = mass in grams/molar mass = 51.3g/28 g/mol = 1.83 mol
xHe = 4.6/(4.6+1.83) = 4.6/6.43 = 0.715
Pt = 40.1 atm
PHe = 0.715 * 40.1 atm = 28.67 atm
Patial pressure of He = 28.7
Explanation / Answer
A 51.3-g sample of N2 (g) is mixed with 18.4 g of He (g) in a container. If the total pressure is 40.1 atm, what is the partial pressure of He? Only enter your numerical answer. Do not enter units.
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