A cylinder is filled with 200 moles of nitrogen, 300 moles of argon, and 5.00 moles of helium. If the gas mixture is at STP, what is the partial pressure of the argon?

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A cylinder is filled with 200 moles of nitrogen, 300 moles of argon, and 5.00 moles of helium. If the gas mixture is at STP, what is the partial pressure of the argon?

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Answer 1 · 2016-12-17T08:31:27

The $partial pressure$ $"partial pressure"$ of any gaseous mixture is simply proportional to its mole fraction.

Explanation:

$P_{Ar} = \frac{n_{Ar}}{n_{dinitrogen} + n_{Ar} + n_{He}} \times P_{gaseous mixture}$ $P_"Ar"=n_"Ar"/(n_"dinitrogen"+n_"Ar"+n_"He")xxP_"gaseous mixture"$

$= \frac{300 \cdot m o l}{200 \cdot m o l + 300 \cdot m o l + 5 \cdot m o l} \times 1 \cdot bar$ $=(300*mol)/(200*mol+300*mol+5*mol)xx1*"bar"$

$= \frac{300}{505} \times 1 \cdot bar$ $=300/505xx1*"bar"$

I leave ti to you to decide what is $S T P$ $STP$ . Different syllabus has different requirements.

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A cylinder is filled with 200 moles of nitrogen, 300 moles of argon, and 5.00 moles of helium. If the gas mixture is at STP, what is the partial pressure of the argon?

1 Answer

Explanation:

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