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

In summary, using the ideal gas law and mole fraction equation, we can calculate the initial partial pressures of nitrogen and oxygen in a cylinder containing 1 L of air at 10 atm and 298 K. With the knowledge that air is composed of 79% nitrogen and 21% oxygen by volume, we can find the respective mole fractions and use them to calculate the partial pressures of each gas. Avogadro's law states that 1 mol of every gas occupies the same volume at the same pressure and temperature, which helps in determining the mole fractions.
  • #1
Ahalp
11
0

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.
 
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  • #2
What does Avogadro's law say about moles & volumes?
 
  • #3
1 mol of every gas occupies the same volume (at the same pressure and temperature).

Thanks, it makes sense now :)
 

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

1. What is partial pressure of air?

Partial pressure of air refers to the pressure exerted by a single gas in a mixture of gases. In other words, it is the pressure that a gas would exert if it occupied the same volume as the entire mixture at the same temperature.

2. How is partial pressure of air calculated?

Partial pressure of air can be calculated by multiplying the total pressure of the gas mixture by the mole fraction of the specific gas. The mole fraction is the ratio of the moles of the specific gas to the total moles of all gases in the mixture.

3. What factors affect the partial pressure of air?

The partial pressure of air is affected by the temperature, total pressure of the gas mixture, and the mole fraction of the specific gas. Changes in any of these factors can result in a change in the partial pressure of the specific gas.

4. Why is partial pressure of air important?

Partial pressure of air is important in many scientific fields, including chemistry, biology, and environmental science. It helps determine the concentration of a specific gas in a mixture and plays a role in gas exchange processes, such as respiration and photosynthesis.

5. How is partial pressure of air measured?

Partial pressure of air can be measured using various instruments, such as a barometer or a manometer. These instruments measure the pressure exerted by a specific gas in a mixture and can be used to calculate the partial pressure. In laboratory settings, gas chromatography is often used to measure the partial pressure of different gases in a mixture.

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