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Dalton’s Law of Partial Pressures - Understanding Atmospheric Pressure and Gas Mixtures

Learn about Dalton’s Law of Partial Pressures and how it applies to atmospheric pressure and gas mixtures. Discover how to calculate partial pressures and determine the composition of gases in the air.

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Dalton’s Law of Partial Pressures - Understanding Atmospheric Pressure and Gas Mixtures

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  1. Chapter 18 Dalton’s Law of Partial Pressures

  2. We all live in the ocean of air, called the atmosphere.

  3. Barometers and Standard Atmospheric Pressure

  4. Barometers and Standard Atmospheric Pressure • Standard atmospheric pressuredefined as the pressure sufficient to support a mercury column of 760mm high. (units of mmHg, or torr). • Another unit was introduced to simplify things, the atmosphere (1 atm= 760 mmHg). • 1 atm = 760 mmHg = 760 torr = 101.3 kPa.

  5. STP standard temperature and pressure Standard temperature0°C or 273 K Standard pressure1 atm (or equivalent)

  6. Dalton’s Law of Partial Pressure • The total pressure of a mixture of gases is the sum of the partial pressures of all the gases in the container. • In a gaseous mixture, a gas’s partial pressure is the one the gas would exert if it were by itself in the container. • Ptotal = P1 + P2 + P3 • Ptotal = 100 kPa + 250 kPa + 200 kPa = 550 kPa 550 kPa A

  7. Turn to the “Dalton’s Law of Partial Pressures” sheet in your notebook.

  8. Air is composed primarily of four gases: nitrogen (593.4 torr), argon (7.098 torr), carbon dioxide (0.2508 torr), and oxygen. What is the partial pressure of oxygen at standard atmospheric pressure? • 593.4 torr + 7.098 torr + 0.2508 torr = 600.7488 torr ≈ 600.7 torr • 760 torr – 600.7 torr = 159.3 torr ≈ 159 torr

  9. Air is composed primarily of four gases: nitrogen (593.4 torr), argon (7.098 torr), carbon dioxide (0.2508 torr), and oxygen. What percent of air is nitrogen? 593.4 torr 760 torr x 100 = 78.1%

  10. Air is composed primarily of four gases: nitrogen (593.4 torr), argon (7.098 torr), carbon dioxide (0.2508 torr), and oxygen. What is the partial pressure in kPa of argon gas at standard atmospheric pressure? 7.098 torr 101.3 kPa = 0.946 kPa 760 torr

  11. What would be the partial pressure of oxygen on top of a high mountain where the air pressure is only 534 mm Hg? Remember from the first problem that the partial pressure of oxygen in air is 159 torr 159 torr X = 760 torr 534 torr x = 112 torr

  12. What percent less oxygen is dissolved into the blood on top of the mountain as compared to sea level? 112 torr x 100 = 70.4% 159 torr 100 – 70.4 = 29.6% less

  13. Mount Everest

  14. Endurance Training

  15. Homework • Dalton’s Law of Partial Pressures Worksheet

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