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Gases Review Quiz: Barometers, Standard Atmospheric Pressure, Boyle's & Charles' Laws

This review quiz covers topics on barometers, standard atmospheric pressure, and gas laws including Boyle's Law and Charles' Law. Learn about pressure-volume relationships and how temperature affects gas volume. Explore the combined gas law and Avogadro's Law, and understand the behavior of ideal gases using the ideal gas equation. Improve your knowledge of gases with this comprehensive quiz.

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Gases Review Quiz: Barometers, Standard Atmospheric Pressure, Boyle's & Charles' Laws

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  1. Chapter 10 Gases

  2. Review Quiz • Net Ionic Equations (includes questions about the reactions).

  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 (units of mmHg, or torr).

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

  6. Barometers and Standard Atmospheric Pressure • Standard atmospheric pressuredefined as the pressure sufficient to support a mercury column of 760mm (units of mmHg, or torr). • Another unit was introduced to simplify things, the atmosphere (1 atm= 760 mmHg). • 1 atm = 760 mmHg = 760 torr = 101.325 kPa (page 262).

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

  8. Boyle’s Law

  9. Boyle's Law • Pressure varies inversely with the volume of a sample of gas if temperature remains constant.”

  10. Boyle’s Law

  11. Boyle’s Law: Pressure & Volume

  12. A sample of air occupies 73.3 mL at 98.7 atm and 0 ºC. What volume will the air occupy at 4.02 atm and 0 ºC? Boyle’s Law: Pressure-Volume Relationships 1800 mL

  13. A sample of helium occupies 535 mL at 988 mmHg and 25 °C. If the sample is transferred to a 1.05-L flask at 25 °C, what will be the gas pressure in the flask? Boyle’s Law: Pressure-Volume Relationships 503 mm Hg

  14. Charles' Law • Effects of temperature on a gas • Volume varies directly with Temperature “The volume of a quantity of gas, held at constant pressure, varies directly with the Kelvin temperature.”

  15. Charles’s Law a

  16. Charles Law: Volume and Temperature (Figure 10.8 Page 266)

  17. Charles’ Law and Absolute Zero • Extrapolation to zero volume gives a temperature of -273°C or 0 K

  18. Charles’s Law: Temperature-Volume Relationships A sample of oxygen gas occupies a volume of 2.10 L at 25 °C. What volume will this sample occupy at 150 °C? (Assume no change in pressure.) 2.98 L

  19. Charles’s Law: Temperature-Volume Relationships A sample of oxygen gas occupies a volume of 2.10 L at 25 °C.At what Celsius temperature will the volume of oxygen occupy 0.750 L? (Assume no change in pressure.) -167°C

  20. Pressure varies directly with Temperature If the temperature of a fixed volume of gas doubles its pressure doubles. Pressure vs. Temperature

  21. Pressure vs. Temperature • The pressure exerted by a gas is directly related to the Kelvin temperature. • V is constant.

  22. Pressure vs. Temperature

  23. Example A gas has a pressure of 645 torr at 128°C. What is the temperature in Celsius if the pressure increases to 1.50 atm? Pi = 645 torr Pf = 1.50 atm 760 torr = 1140 torr 1 atm Ti = 128°C + 273 = 401 K Tf = ?K

  24. Solution T2 = 401 K x 1140 torr = 709K 645 torr 709K - 273 = 436°C

  25. Combined Gas Law Problem A sample of helium gas has a volume of 0.180 L, a pressure of 0.800 atm and a temperature of 29°C. What is the new temperature(°C) of the gas at a volume of 90.0 mL and a pressure of 3.20 atm?

  26. Combined Gas Law Problem A sample of helium gas has a volume of 0.180 L, a pressure of 0.800 atm and a temperature of 29°C. What is the new temperature(°C) of the gas at a volume of 90.0 mL and a pressure of 3.20 atm? x3.20 atmx 90.0 mL 0.800 atm 180.0 mL 604 K - 273 = 331 °C 302 K = 604 K

  27. Combined Gas Law • A 10.0 cm3 volume of gas measured 75.6 kPa and 60.0C is to be corrected to correspond to the volume it would occupy at STP. 6.12 cm3

  28. Gay-Lussac’s Law Gay-Lussac’s Law of combining volumes: at a given temperature and pressure, the volumes of gases which react are ratios of small whole numbers.

  29. How many liters of steam can be formed from 8.60L of oxygen gas? 17.2 L

  30. How many liters of hydrogen gas will react with 1L of nitrogen gas to form ammonia gas? 3L H2

  31. A

  32. A How many mL of hydrogen are needed to produce 13.98 mL of ammonia? 20.97 ml NH3

  33. Avogadro’s Law: Equal volumes of gases at the same temperature and pressure contain the same number of particles.

  34. The molar volume of a gas at STP = 22.4L 22.4 L

  35. Ideal Gas • An ideal gas is defined as one for which both the volume of molecules and forces of attraction between the molecules are so small that they have no effect on the behavior of the gas.

  36. Ideal Gas Equation PV=nRT

  37. R values • A a • I • R values for atm and kPa on Page 272 in book.

  38. Calculate the volume occupied by 0.845 mol of nitrogen gas at a pressure of 1.37 atm and a temperature of 315 K. 15.9 L

  39. Find the pressure in millimeters of mercury of a 0.154 g sample of helium gas at 32°C and contained in a 648 mL container. 1130 mm Hg

  40. Boyle’s Law and Diving • What is more dangerous? • A deep dive or a shallow dive.

  41. Boyle’s Law and Diving • We can answer this by first noting that for every 10 meters you descend in the water, the pressure increases by about 1 atm.

  42. Boyle’s Law and Diving • When you hold your breath, you create a closed system with your lungs and Boyle's law applies. • If you are down at 90 meters (at 10 atm) and you rise 10 meters to 80 meters (at 9 atm), the pressure has decreased by about 10%, and since PV is a constant your lungs expand by about 10% (probably not too bad).

  43. Why is PV is constant? • PV=nRT • The right side of the equation has not changed (we have not changed temperature or the amount of gas in the lungs). • Therefore the left side of the equation, (PV) must remain constant as well.

  44. Boyle’s Law and Diving • Now if you are at 10 meters (at 2 atm), and you rise 10 meters to the surface (at 1 atm) the pressure had decreased by 50% and expanding your lungs by this factor could cause significant damage, maybe death!

  45. An experiment shows that a 113 mL gas sample has a mass of 0.171 g at a pressure of 721 mm Hg and a temperature of 32°C. What is the molar mass (molecular weight) of the gas? 40.0 g/mol

  46. Can the ideal “gas” equation be used to determine the molar mass of a liquid?

  47. Problem: A volatile liquid is placed in a flask whose volume is 590.0 ml and allowed to boil until all of the liquid is gone, and only vapor fills the flask at a temperature of 100.0 oC and 736 mm Hg pressure. If the mass of the flask before and after the experiment was 148.375g and 149.457 g, what is the molar mass of the liquid? 57.9 g/mol

  48. What is the density of methane gas (natural gas), CH4, at 125oC and 3.50 atm? 1.71 g/L

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