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Topic: Partial Pressures  (Read 4222 times)

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Offline TEA1

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Partial Pressures
« on: May 07, 2008, 10:10:48 PM »
1. Ozone concentration is 0.22 ppm by volume.  Calculate the partial pressure of ozone and number of ozone molecules per liter of air if the temperature and pressure were 20.0 C and 738mmHg.
  ---I am not sure what equation to start

2.  Given that the quantity of ozone in the stratosphere is equivilent to a 3.0mm thick layer of ozone on Earth at STP. Calculate the number of ozone molecules in the stratosphere and their mass in kilograms. (Earth radius is 6371 km and surface area of sphere is 4 pie r squared)
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Offline Borek

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Re: Partial Pressures
« Reply #1 on: May 08, 2008, 03:47:33 AM »
Quote from: TEA1 on May 07, 2008, 10:10:48 PM
I am not sure what equation to start

Both partial pressure definition and ideal gas equation will come handy.
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Offline TEA1

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Re: Partial Pressures
« Reply #2 on: May 08, 2008, 11:48:52 AM »
Okay...but I still don't know how that will work for the 2nd question.  I think I understand the 1st question now.
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Offline Borek

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Re: Partial Pressures
« Reply #3 on: May 08, 2008, 12:22:12 PM »
Just find the volume of the gas, then it should be obvious.
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Offline AhmedEzatAlzawalaty

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Re: Partial Pressures
« Reply #4 on: May 08, 2008, 02:25:15 PM »
can any one tell me how to solve problems about calculating gauge pressure inside aerosol container(pharmaceutics) or recommend a good site?
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