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Chapter 11

Chapter 11. Gases. Conditions that affect gases. volume pressure temperature # of particles. Pressure and Force. Pressure = force area Example of pressure:. Pressure. Atmospheric pressure- 14.7 psi 78% nitrogen, 21% oxygen and 1% other gas. Pressure.

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Chapter 11

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  1. Chapter 11 Gases

  2. Conditions that affect gases • volume • pressure • temperature • # of particles

  3. Pressure and Force • Pressure = force area Example of pressure:

  4. Pressure • Atmospheric pressure- 14.7 psi • 78% nitrogen, 21% oxygen and 1% other gas

  5. Pressure • Ways to measure pressure: • Open end manometer • Closed end manometer • Barometer

  6. Pressure

  7. Pressure • Barometer-measures atmospheric pressure

  8. Pressure • Units of Pressure: see pg.364 • Millimeters of mercury • Kilopascals,pascals • atmospheres • torr • 760 mmHg = 1 atm= 101.325 kPa = 760 torr

  9. Pressure Conversions • Examples: • Convert the pressure of 775 mm Hg to kPa and to atm. • Practice: • Convert a pressure of 750. torr to a. Atm b. kPa

  10. Standard Conditions • STP- Standard Temperature and Pressure • Agreed upon standard • 0°C and 1 atm

  11. Dalton’s Law of Partial Pressures • Each individual gas has its own pressure (partial pressure) • Ptotal = Pa + Pb + Pc + …..

  12. Sample problems for Dalton’s Law • Example: Calculate the partial pressure in mm Hg exerted by the four main gases in air: nitrogen, oxygen, argon and carbon dioxide. Their abundance by volume is 78.08%, 20.95%, .934% and .035 % respectively.

  13. Sample problems for Dalton’s Law • Example : In a sample containing carbon dioxide, nitrogen and oxygen at exactly 1 atm. The partial pressure of CO2 is .285 torr and the partial pressure of N2 is 593.525 torr. What is the partial pressure of O2?

  14. Dalton’s Law of Partial Pressures • Collecting gas over water: • -useful for gases that do not dissolve or react with water • - water has a partial pressure, it increases with increased temp. • -must use a table for the exact value pg. 859 • Patm = Pgas + PH20

  15. Dalton’s Law of Partial Pressures

  16. Sample problems for Dalton’s Law • Example: Oxygen gas was collected from the decomposition of potassium chlorate. The atmospheric pressure was 731.0 torr and the temperature of the water was 20.0 C. What was the partial pressure of the oxygen gas collected?

  17. Sample problems for Dalton’s Law • Practice: A sample of nitrogen gas is collected over water at a temperature of 23.0 °C. What is the pressure of the nitrogen gas if the atmospheric pressure is 785 mm Hg?

  18. The Simple Gas Laws • Boyle’s Law • Charles’s Law • Gay-Lussac’s Law • The Combined Gas Law

  19. Boyle’s Law • When temp. and # of particles are constant the pressure and volume of a gas are inversely proportional • P1V1= P2V2

  20. Boyle’s Law -practice • Example: A sample of gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be at a pressure of 0.987 atm if the pressure and amount of gas remain constant? • Practice: A helium filled balloon contains 125 mL of gas at a pressure of .974 atm What volume will the gas occupy at standard pressure?

  21. Charles’s Law • With constant amount of gas and pressure the volume and temperature of a gas will have a directly proportional relationship • V1 = V2 T1 T2 • NOTE: TEMPERATURE MUST BE IN KELVIN • K= ° C + 273

  22. Charles's Law Practice • Example: A sample of neon gas occupies a volume of 752 mL at 25 ° C. What volume will the gas occupy at 50° C if the pressure remains constant? • Practice: A balloon filled with oxygen gas occupies a volume of 5.5 L at 25° C. What volume will the gas occupy at 100. ° C?

  23. Gay-Lussac’s Law • Pressure and temperature of a gas are directly proportional if the amount and volume of gas remain constant • P1= P2 T1 T2

  24. Gay-Lussac’s Law Practice • Example: The gas in an aerosol can is at a pressure of 3.00 atm at 25°C. What would the pressure of the gas be if the can was heated to 52° C? • Practice: The temperature within a car tire at the beginning of a long trip is 25° C. At the end of the trip the tire has a pressure of 1.80 atm. What is the final temperature within the tire if its original pressure was 1.75 atm?

  25. The Combined Gas Law • Expresses all of the simple gas laws, relating temperature, pressure and volume of a gas as long as the amount of gas remains constant. • P1V1 = P2V2 T1 T2 • MEMORIZE this law, cross out the factors that remain constant.

  26. The Combined Gas Law Practice • Example:A helium filled balloon has a volume of 50.0L at 25° C and 1.08 atm. What will the new volume be if its pressure is decreased to .855 atm and the temperature decreases to 10. ° C? • Practice: The volume of a gas at 27.0 ° C and .200 atm is 80.0 mL. What volume will the same gas sample occupy at standard conditions?

  27. END of MATERIAL FOR TEST 1

  28. Measuring and Comparing the Volumes of Reacting Gases • Law of Combining Volumes • at constant temperature and pressure, the volumes of gases react and can be expressed as whole numbers • Try this: Write and balance and equation for each. • hydrogen gas and oxygen gas produces water vapor • hydrogen gas and chlorine gas produce hydrogen chloride gas Now go to pg.378 and check the results

  29. Measuring and Comparing the Volumes of Reacting Gases • Avogadro’s Law • Equal volumes of gases at the same temperature and pressure contain equal # of molecules • standard molar volume of a gas • one mole of any gas at STP = 22.4L of that gas

  30. Measuring and Comparing the Volumes of Reacting Gases • Example: at STP • 2H2(g) + O2(g)  2H2O(g) • __ L __ L __ L • 2 mL 1 mL 2 mL • __ molecules__ molecule __ molecules • __ moles 1 mole __ moles • 44.8 L 22.4 L __ L

  31. Using Molar Volume of a Gas • You are planning an experiment that requires .0580 mol of nitrogen monoxide gas. What volume would you need at STP? • Practice: A chemical reaction produces .0680 mol of oxygen gas. What volume in liters is occupied by this gas at STP?

  32. Using Molar Volume of a Gas • Challenge: Suppose you need 4.22 g of chlorine gas,Cl2. What volume at STP would you expect to use?

  33. Stoichiometry of Gases • - if constant temp and pressure, just use the molar ratio from the equation!! • - volume and moles are the same ratio as the equation!!

  34. Stoichiometry of Gases • Example:Propane is C3H8. • Write the combustion reaction for propane. • a. What will be the volume, in liters of oxygen required for the complete combustion of .350 L of propane? Assume STP • b. What will be the volume of carbon dioxide produced in the same reaction starting with .350 L of propane? Assume STP

  35. Stoichiometry of Gases • Practice: Xenon gas reacts with fluorine gas to produce the gas xenon hexafluoride. Write the equation for this reaction. • a. Assuming constant temperature and pressure, what volume of xenon should be used to make 3.14 L of XeF6? • b. What volume of fluorine gas should be used to create 3.14 L of XeF6?

  36. The Ideal Gas Law • includes, temperature, pressure, volume and # of moles • single conditions, not P1,P2 • PV= nRT

  37. PV=nRT • P= pressure (must match unit of pressure in R value) • V= volume (must be in L) • N= # of moles (convert to moles if given grams) • T= temperature (Kelvin) • R= ideal gas law constant • R= .0821 L . atm mol.K • See various numerical values for R on pg. 384

  38. Ideal Gas Law Practice • Example: What is the pressure in atm exerted by a .500 mol sample of nitrogen gas in a 10.0L container at 298K? • Practice: A 2.07 L cylinder contains 2.88 mol of helium gas at 22° C. What is the pressure in atm of the gas in the cylinder? (P= 33.7 atm)

  39. Ideal Gas Law Practice • Practice: A tank of hydrogen gas has a volume of 22.9 L and holds 14.0 mol of the gas at 12° C. What is the reading on the pressure gauge in mm Hg?(14.3 atm1.09X104 mmHg) • Practice: A reaction yields 0.00856 mol of oxygen gas. What volume in mL will the gas occupy if it is collected at 43 °C and .926 atm? (.240 L240. mL)

  40. Effusion and diffusion • lighter molecules move faster • Graham’s Law of Effusion-the rate of effusion and diffusion is inversely proportional to the square root of the molecular weights of the gases

  41. Graham’s Law Practice • Example: Nitrogen gas effuses through a pinhole 1.7 times as fast as another element under the same conditions. Estimate the other element’s mass and determine its probable identity.

  42. Graham’s Law Practice • Practice: Compare the rates of effusion of hydrogen and oxygen gas at the same conditions. (Remember, both are diatomic.)

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