What is the Partial Pressure of Air in a Cylinder at 10 atm and 298 K?

AI Thread Summary
To calculate the partial pressures of nitrogen (N2) and oxygen (O2) in a cylinder containing air at 10 atm and 298 K, the ideal gas law (PV = nRT) and the concept of mole fractions are essential. Given that air is 79% N2 and 21% O2 by volume, the mole fractions can be directly derived from these percentages. Using the formula for partial pressure (Pi = yi P), the partial pressure of N2 is 7.9 atm and that of O2 is 2.1 atm. Understanding that volume ratios correspond to mole ratios under the same conditions simplifies the calculation. This approach effectively clarifies how to determine the partial pressures based on the composition of air.
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Homework Statement



A cylinder contains 1 L of air at 10 atm and 298 K.
Knowing that air is composed of 79% N2 and 21% O2 by VOLUME, calculate the initial partial pressure for both.

Homework Equations



Ideal Gas Law: PV = nRT

Mole Fraction: yi = moles of i / total moles

Partial Pressure: Pi = yi P

The Attempt at a Solution



The main thing throwing me off is that the composition is by Volume, not mass or moles.
I'm completely stumped on how to find the mole fractions.
 
Physics news on Phys.org
What does Avogadro's law say about moles & volumes?
 
1 mol of every gas occupies the same volume (at the same pressure and temperature).

Thanks, it makes sense now :)
 
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