Question

A sample of the atmosphere at a total pressure of 740. mm Hg is analyzed to give these partial pressures: 1. P (N2) = 575 mm Hg 2. P (Ar) = 6.90 mm Hg 3. P (CO2) = 0.20 mm Hg 4. P (H2O) = 4.0 mm Hg No other gases except O2 have appreciable partial pressures. a) What is the partial pressure of O2? b) What is the mole fraction of each gas?

          A sample of the atmosphere at a total pressure of 740. mm Hg is analyzed to give these partial pressures:

1. P (N2) = 575 mm Hg
2. P (Ar) = 6.90 mm Hg
3. P (CO2) = 0.20 mm Hg
4. P (H2O) = 4.0 mm Hg

No other gases except O2 have appreciable partial pressures.
a) What is the partial pressure of O2?
b) What is the mole fraction of each gas?

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$A sample of the atmosphere at a total pressure of 740. mm Hg is analyzed to give these partial pressures: 1. P (N2) = 575 mm Hg 2. P (Ar) = 6.90 mm Hg 3. P (CO2) = 0.20 mm Hg 4. P (H2O) = 4.0 mm Hg No other gases except O2 have appreciable partial pressures. a) What is the partial pressure of O2? b) What is the mole fraction of each gas?$

Added by Christopher H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

09/20/2023

Step 1

We know that the total pressure is the sum of the partial pressures of all the gases. So, we can write: Total Pressure = P(N₂) + P(Ar) + P(CO₂) + P(H₂O) + P(O₂) Now, we can plug in the given values and solve for P(O₂): 740 mm Hg = 575 mm Hg + 6.90 mm Hg + 0.20 Show more…

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A sample of the atmosphere at a total pressure of 740. mm Hg is analyzed to give these partial pressures: 1. P (N2) = 575 mm Hg 2. P (Ar) = 6.90 mm Hg 3. P (CO2) = 0.20 mm Hg 4. P (H2O) = 4.0 mm Hg No other gases except O2 have appreciable partial pressures. a) What is the partial pressure of O2? b) What is the mole fraction of each gas?

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