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The Gas Laws

JEOPARDY REVIEW. The Gas Laws. Jeopardy Categories. 100. 100. 100. 100. 100. 100. 200. 200. 200. 200. 200. 200. 300. 300. 300. 300. 300. 300. 500. 500. 500. 500. 500. 500. 1000. 1000. 1000. 1000. 1000. 1000. Boyle’s Law- $100.

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The Gas Laws

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  1. JEOPARDY REVIEW The Gas Laws

  2. Jeopardy Categories 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 500 500 500 500 500 500 1000 1000 1000 1000 1000 1000

  3. Boyle’s Law- $100 According to Boyle’s Law, the volume of a gas varies ____________ (directly or inversely) with its pressure, assuming that temperature is constant. INVERSELY BACK

  4. Boyle’s Law- $200 According to Boyle’s Law, the volume of a gas ______________ (increases, decreases, or stays the same) when the pressure increases and temperature is held constant. DECREASES BACK

  5. Boyle’s Law- $300 A sample of oxygen gas at constant temperature occupies a volume of 250. mL at 740. torr pressure. What volume in mL will it occupy at 800. torr pressure? BACK

  6. Boyle’s Law- $500 Ammonia gas occupies a volume of 450. mL at a pressure of 720. mm Hg. What volume in mL will it occupy at standard pressure? BACK

  7. Boyle’s Law- $1000 Fluorine gas has a volume of 317 mL. When the volume is decreased to 250. mL, its pressure is 1.50 atm. What was the original pressure in torr? BACK

  8. CHARLES $100 According to Charles’ Law, the volume of a gas varies ____________ (directly or inversely) with the Kelvin temperature, assuming that pressure is constant. DIRECTLY BACK

  9. CHARLES - $200 According to Charles’ Law, the volume of a gas ______________ (increases, decreases, or stays the same) when the temperature increases and pressure is held constant. INCREASES BACK

  10. CHARLES - $300 A sample of nitrogen occupies a volume of 0.250 L at 298 K. What volume in liters will it occupy at 368 K? BACK

  11. CHARLES - $500 Hydrogen gas was cooled from 423K to 323K. Its new volume is 0.075 liters. What was its original volume? BACK

  12. CHARLES - $1000 A sample of argon gas is cooled and its volume decreased from 0.380 mL to 0.250 mL. If its final temperature was 218 K, what was its original temperature in degrees Celsius? BACK

  13. Combined - $100 What are the three variables in the Combined Gas Law? VOLUMEPRESSURETEMPERATURE BACK

  14. Combined - $200 P1 = 1.5 atm P2 = 2.5 atm V1 = 3.0 L V2 = ? T1 = 293 K T2 = 303 K BACK

  15. Combined - $300 P1 = 720. torr P2 = ? V1 = 0.256 L V2 = 0.250 L T1 = 298 K T2 = 323 K BACK

  16. Combined - $500 P1 = 95.0 kPa P2 = 101kPa V1 = 4.00 L V2 = 6.00 L T1 = ? T2 = 471 K BACK

  17. Combined - $1000 A gas has an initial volume of 125 mL and pressure of 125 kPa. When its volume is decreased to 100. mL and its pressure is decreased to 100. kPa, its temperature is changed to 348 K. What is the initial temperature of this gas in K? BACK

  18. PV=nRT - $100 Why must pressure be in atmospheres, volume be in liters, and temperature be in Kelvin when using the constant with a numerical value of 0.0821? Because the Universal Gas Constant, R, that has a value of 0.0821 has a unit of (L•atm)/(mol•K). The units must be consistent or they will not cancel out. BACK

  19. PV=nRT - $200 How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 298 K? BACK

  20. PV=nRT - $300 What volume will 2.0 moles of nitrogen occupy at 0.947 atm and 293 K? BACK

  21. PV=nRT - $500 At what temperature will 0.70 mol of chlorine gas exert a pressure of 900. torr of pressure at a and a volume of 500. mL? BACK

  22. PV=nRT - $1000 An elemental gas has a mass of 10.3 g. If the volume is 58,400 mL and the pressure is 758 mm Hg at a temperature of 2.5°C, how many moles are present? What is the gas? BACK

  23. GRAHAM - $100 Graham’s Law allows a scientist to make predictions about what property of gases if the molecular masses are known? Rates of EFFUSION BACK

  24. GRAHAM - $200 According to Graham’s Law, a gas will effuse at a rate that is _____________ proportional to the square root of its molecular mass. INVERSELY BACK

  25. GRAHAM - $300 Based on molecular masses, which will effuse faster: Hydrogen or Oxygen BACK

  26. GRAHAM - $500 Arrange the following gases in order of increasing rates of effusion (slowest to fastest): NH3, CO2, He, Cl2 BACK

  27. GRAHAM - $1000 Under the same conditions of temperature and pressure, what is the relative rate of effusion of oxygen gas effuse compared to hydrogen gas? BACK

  28. DALTON - $100 Dalton’s Law says that the sum of the individual pressures of all the gases that make up a mixture is equal to the ___________ ___________. TOTAL PRESSURE BACK

  29. DALTON - $200 The partial pressures of a gas are 22.1 torr, 168 torr, and 33.0 torr. What is the total pressure of this gas? BACK

  30. DALTON - $300 A 250. mL sample of oxygen is collected over water at 25.0°C and 760.0 torr pressure. What is the pressure of the dry gas alone? (Vapor pressure of water at 25.0 °C = 23.8 torr) BACK

  31. DALTON - $500 A mixture of 2.00 moles of hydrogen, 3.00 moles of ammonia, 4.00 moles of carbon dioxide, and 5.00 moles of nitrogen exerts a total pressure of 800. torr. What is the partial pressure in torr of carbon dioxide? BACK

  32. DALTON - $1000 What element is used when discussing units of pressure in mm? (pressure= mm ____ ) Mercury ; Hg BACK

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