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To prevent air from interacting with highly reactive chemicals, noble gases are placed over the chemicals to act as inert “blanketing” gases. A chemical engineer places a mixture of noble gases consisting of 5.50 g of He, 15.0 g of Ne, and 35.0 g of Kr in a piston-cylinder assembly at STP. Calculate the Partial Pressure per Gas​

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Explanation:

Given parameters:

Mass of He  = 5.5g

Mass of Ne  = 15g

Mass of Kr  = 35g

Pressure at STP = 1atm

Unknown:

Partial pressure per gas = ?

Solution:

Partial pressure is the pressure a gas would exert it alone occupies the container.

 Partial pressure of a gas  = Mole fraction of a gas x Total pressure of mixture

        Number of moles  = [tex]\frac{mass}{molar mass}[/tex]

Number of moles of He  = [tex]\frac{5.5}{4}[/tex]   = 1.375mole

Number of moles of Ne = [tex]\frac{15}{20}[/tex]   = 0.75mole

Number of moles of Kr = [tex]\frac{35}{83.8}[/tex]  = 0.42mole

Sum total of moles  = 1.375 + 0.75 + 0.42 = 2.54moles

Partial pressure of He  = [tex]\frac{1.375}{2.54}[/tex] x 1atm = 0.54atm

Partial pressure of Ne = [tex]\frac{0.75}{2.54}[/tex] x 1atm  = 0.29atm

Partial pressure of kr  = [tex]\frac{0.42}{2.54}[/tex] x 1atm = 0.17atm

Given parameters:

  • Mass of He  = 5.5g
  • Mass of Ne  = 15g
  • Mass of Kr  = 35g
  • Pressure at STP = 1atm

Formula:

Partial pressure of a gas  = Mole fraction of a gas x Total pressure of mixture

Number of moles  = Mass/Molar Mass

  • Number of moles of He  =  5.5/4  = 1.375mole
  • Number of moles of Ne = 15/20   = 0.75mole
  • Number of moles of Kr =35/83.8   = 0.42mole

Sum total of moles  = 1.375 + 0.75 + 0.42

Sum total of moles  = 2.54moles

  • Partial pressure of He  = 1.375/2.54 x 1atm = 0.54atm
  • Partial pressure of Ne = 0.75/2.54 x 1atm  = 0.29atm
  • Partial pressure of kr  =0.42/2.54  x 1atm = 0.17atm

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