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IRISSAK [1]
2 years ago
14

You have a mixture of the gases Cl₂ and O₂ along with some N₂ in a container at STP. The moles of Cl₂ and O₂ in the mixture are

equivalent and the density of the mixture is 2.063 g/L. Assuming ideal behavior, what is the mole fraction of N₂ in the mixture?
Chemistry
1 answer:
Harman [31]2 years ago
8 0

The mole fraction of N₂ in the mixture, given the data is 0.225

<h3>How to determine the mass of the mixture</h3>
  • Density of mixture = 2.063 g/L
  • Volume (at STP) = 22.4 L
  • Mass of mixture =?

Density = mass / volume

Cross multiply

Mass = Density × volume

Mass of mixture = 2.063 × 22.4

Mass of mixture = 46.2112 g

<h3>How to determine the mole fraction of N₂</h3>

We'll begin by calculating the mole of N₂ in the mixture. This can be obtained as follow:

  • Mass of mixture = 46.2112 g
  • Let the mole of Cl₂ = y
  • Let the mole of O₂ = Mole of Cl₂ = y
  • Total mole = 1 mole
  • Let the mole of N₂ = x =?

Total mole = Mole of N₂ + Mole of Cl₂ + Mole of O₂

1 = x + y + y

1 = x + 2y

2y = 1 - x

y = (1 - x) / 2

Mass of mixture = mass of N₂ + mass of Cl₂ + mass of O₂

Recall

mass = mole × molar mass

Thus,

Mass of mixture = (mole of N₂ × molar mass) + (mole of Cl₂ × molar mass) + (mole of O₂ × molar mass)

46.2112 = 28x + 71y + 32y

But

y = (1 - x) / 2

46.2112 = 28x + 71(1 - x) / 2 + 32(1 - x) / 2

Multiply through by 2

92.4224 = 56x + 71(1 - x) + 32(1 - x)

92.4224 = 56x + 71 - 71x + 32 - 32x

Collect like terms

92.4224 - 71 - 32 = 56x - 71x - 32x

-10.5776 = -47x

Divide both sides by -47

x = -10.5776 / -47

x = 0.225 mole

Finally, we can determine the mole fraction of N₂. This can be obtained as follow:

  • Mole of N₂ = x = 0.225 mole
  • Total mole = 1 mole
  • Mole fraction of N₂ = ?

Mole fraction = mole / total mole

Mole fraction of N₂ = 0.225 / 1

Mole fraction of N₂ = 0.225

Learn more about mole fraction:

brainly.com/question/2769009

#SPJ1

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