A mixture of xenon and hydrogen gases, at a total pressure of 675 mm Hg, contain

Question

A mixture of xenon and hydrogen gases, at a total pressure of 675 mm Hg, contains 15.8 grams of xenon and 0.194 grams of hydrogen. What is the partial pressure of each gas in the mixture?

PXe = _____mm Hg
PH2 = _____mm Hg

A mixture of carbon dioxide and neon gases contains carbon dioxide at a partial pressure of 288 mm Hg and neon at a partial pressure of 330 mm Hg. What is the mole fraction of each gas in the mixture?

XCO2 = ______
XNe = _______

A mixture of neon and xenon gases at a total pressure of 836 mm Hg contains neon at a partial pressure of 575 mm Hg. If the gas mixture contains 4.06 grams of neon, how many grams of xenon are present?

_______g Xe

Explanation / Answer

A)

Molecular weight of xenon = 131.3

Molecular weight of Hydrogen = 2

No. of moles of Xe = 0.12

No. of moles of H2 = 0.097 moles

Partial Pressure of Xe = 0.12/(0.12 + 0.097) * 675
= 373.27 mm of Hg

Partial Pressure of H2 = 0.097/(0.12 + 0.097) *675
= 301.73 mm of Hg

B)

P(partial) = X*P(total)

For CO2:

288 = X* (288 + 330)

X(CO2) = 0.466

For Ne :

330 = X * (288 + 330)

X(Ne) = 0.534

C)

X(Ne) = 575/836
= 0.687

Hence;

X(Xe) = 1-0.687
= 0.313

Let the weight of Xe be x:

0.313 = (x/131.2)/(4.06/20 + x/131.2)

Solving this we get;

x = 12.13

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.