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Gases

Gases. DENSITY PARTIAL PRESSURE. Objectives Today I will be able to: Derive the ideal gas law and Dalton’s law of partial pressure to solve gas law problems Explain why gases deviate from the ideal gas law

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Gases

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  1. Gases DENSITY PARTIAL PRESSURE

  2. Objectives • Today I will be able to: • Derive the ideal gas law and Dalton’s law of partial pressure to solve gas law problems • Explain why gases deviate from the ideal gas law • Informal assessment – monitoring student questions as they complete the practice problems • Formal assessment – analyzing student answers to the practice problems and the exit ticket • Common Core Connection • Reason abstractly and quantitatively • Make sense of problems and persevere in solving them

  3. Lesson Sequence • Evaluate: Warm Up • Explain: Partial Pressure Problems • Elaborate: Partial Pressure Practice • Explain: Deviations from the Ideal Gas Law • Elaborate: Van Der Waal’s Practice • Evaluate: Exit Ticket

  4. Warm Up • Get a textbook to share with your row! • A mixture of gases contains 10.25 g of N2, 1.83 g of H2 and 7.85 g of NH3. If the total pressure of the mixture is 1.85 atm, what is the partial pressure of each component? • Which of the following gases behaves most like an ideal gas? Why? • A nonpolar gas at high pressure • A nonpolar gas at low pressure • A polar gas at high pressure • A polar gas at low pressure

  5. Objectives • Today I will be able to: • Derive the ideal gas law and Dalton’s law of partial pressure to solve gas law problems • Explain why gases deviate from the ideal gas law

  6. Homework • Study for Organic Quiz on Wednesday, September 10 • Polyatomic Ions Quiz Thursday, September 11 • Solubility Rules Quiz Thursday, September 18 • Bring lab notebook to school Thursday

  7. Agenda • Warm Up • Review Organic Functional Groups • Review Exam • Gas Law Practice Problems • Exit Ticket

  8. Collecting Gas Over Water: Partial Pressure

  9. http://youtu.be/pgTTKYhqQY0

  10. Collect Gas over Water • http://youtu.be/E5NBZgQ5cl0

  11. http://youtu.be/D2-DtoSQ1Rc

  12. Ideal Gas Law Deviations VAN DER WAALS EQUATION

  13. Deviations from the Ideal Gas Law • The effect of pressure on the behavior of several gases (300 K)

  14. Deviations from the Ideal Gas Law • The effect of temperature and pressure on the behavior of nitrogen gas

  15. Why do real gases deviate from ideal behavior? • Ideal gas law is based on the assumption that ideal gases occupy no space and have no attractions to one another • Real molecules have finite volumes, and they do attract one another

  16. Factors Impacting a Non ideal Gas • Pressure on volume of gas molecules • Attractive forces on pressure of the gas • Temperature’s impact on the attractive forces

  17. Van der Waals Equation • Used by scientists/engineers who work with gases at high pressures and cannot use the ideal gas law • Derived two constants: • a = corrects for attractive forces • b = corrects for the volume the gas occupies itself • Constants are experimentally determined for each gas (Table 10.3 in textbook)

  18. Sample Problem • Consider a sample of 1.000 mol of CO2(g) confined to a volume of 3.000 L at 0.0oC. Calculate the pressure of the gas using (a) the ideal – gas law equation and (b) the van der Waals equation.

  19. Extra Gas Law Practice (Chapter 10) • Partial Pressure • 10.61, 10.68

  20. Exit Ticket • Rearrange the ideal gas law equation to solve for density • Rearrange the ideal gas law equation to solve for molar mass.

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