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Unit 9 Review

Unit 9 Review. Gases. The Game Board. 1. Calculate the approximate volume of a 2.50 mol sample of gas at -8.0°C and a pressure of 3.50 atm. 15.5 L (PV=nRT). Back. 2. In the reaction N 2 (g) + 3H 2 --> 2NH 3 (g), the volume ratio of H 2 to N 2 is___________. 3 to 1 (Coefficients).

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Unit 9 Review

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  1. Unit 9 Review Gases

  2. The Game Board

  3. 1 Calculate the approximate volume of a 2.50 mol sample of gas at -8.0°C and a pressure of 3.50 atm. 15.5 L (PV=nRT) Back

  4. 2 In the reaction N2 (g) + 3H2 --> 2NH3 (g), the volume ratio of H2 to N2 is___________ 3 to 1 (Coefficients) Back

  5. 3 A pressure of 165 kPa is equal to _____ atm. 1.63 Back

  6. 4 What does the constant bombardment of gas molecules against the inside of a container cause? Pressure Back

  7. 5 What happens to the volume of a gas during compression? The Volume Decreases Back

  8. 6 A sample of a gas has a pressure of 2.25 atm, a volume of 650 mL and a temperature of 36°C. What would the volume of the gas be if the pressure is increased to 3.20 atm and the temperature is decreased to 31°C? 449.6 mL (PTV Chart) Back

  9. 7 What temperature is needed to pressurize a 27.3 L container with 6.34 moles of air to 564.8 kPa? 292.5 K (PV=nRT) Back

  10. 8 When pressure, volume, and temperature are known, the ideal gas law can be used to calculate ______________. Molar amount (moles) Back

  11. 9 According to the diagram to the right, what PV/nRT value do ideal gases have all the time? 1.0 Back

  12. 10 What is the SI unit of pressure? Pascal Back

  13. 11 If a gas with an odor is released in a room, it quickly can be detected across the room because it ______________. Diffuses Back

  14. 12 A pressure of 355000 Pa is equal to _____ psi. 51.5 Back

  15. 13 The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to ________________. Avogadro Back

  16. 14 Nitrogen reacts with hydrogen to make ammonia [N2 (g) + 3H2 (g) --> 2NH3 (g)]. If one needs to produce 4 L of ammonia, how many liters of nitrogen are needed? 2 L Back

  17. 15 A sample of a gas occupies a volume of 1.1 L at 33°C. What temperature is needed to increase the volume of the gas to 1.9 L, if the pressure remains constant? 528.5 K or 255°C (PVT Chart) Back

  18. 16 A 10.5 L sample of a gas has a mass of 95.9 g at 7.6 atm and 35°C. What is the molar mass of the gas? (Hint: divide the given mass by n). 30.4 g/mol (PV=nRT) Back

  19. 17 According to the diagram to the right, at what pressure do all the gases most resemble an ideal gas? Back 0 atm

  20. 18 A pressure of 560 mmHg is equal to _____ kPa. 74.7 Back

  21. 19 Who is accredited with the idea that in a reaction, two volumes of hydrogen gas will combine with one volume of oxygen gas to produce two volumes of water vapor? Gay-Lussac Back

  22. 20 The pressure of each gas in a mixture is called the ____________________ pressure. Partial Back

  23. 21 A sample of a gas has a pressure of 567 mmHg at 23°C. What would the gas pressure be at 41°C, if the volume remains constant? 601 mmHg (PTV Chart) Back

  24. 22 To two decimal places, what will vA/vB be equal to if N2 is considered to be gas A and NO is considered to be gas B. (A diffusion problem) 1.03 (Diffusion) Back

  25. 23 Standard temperature and pressure for a gas is ____________________ 0°C and 1 atm. Back

  26. 24 The total pressure of a system of four gases is 35 atm. The first gas has a pressure of 5 atm. The second gas has a pressure of 8 atm. The remaining two pressures are the same. What is the partial pressure of the other two gases? 11 (Dalton’ Law) Back

  27. 25 Charles’s law is the direct relationship between ____________________ and volume. Temperature Back

  28. 26 What is the molar mass of a gas if it diffuses at a rate of 258 m/s while Iodine gas diffuses at 125 m/s at the same temperature? 29.7 g/mol (Diffusion) Back

  29. 27 2H2O(l) + electricity  2H2(g) + O2(g) What mass of H2O is needed to create 15.64 L of O2, if the temperature is 25°C and the pressure is 1.2 atm? 27.6 g (PV=nRT with Stoichiometry) Back

  30. 28 The average kinetic energy of random motion is proportional to the temperature in what unit? Kelvin Back

  31. 29 A sample of oxygen occupies 350 mL when the pressure is 5 atm. At constant temperature, what volume does the gas occupy when pressure falls to 3 atm? 583 mL (PTV Chart) Back

  32. 30 Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures? Dalton Back

  33. 31 What is the theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system? Kinetic Molecular Theory Back

  34. 32 A mixture of gases with a pressure of 800.0 mm Hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure of oxygen in this mixture? 320 mm Hg Back

  35. 33 Line D represents water. If the atmospheric pressure in a flask is lowered to 70 kPa, water would boil at what temperature? 92 C Back

  36. 34 T1 = 76 C P1 = 4 atm V1 = 560 mL T2 = 92 C P2 = 2 atm V2 = ? 1171 mL (PTV Chart) Back

  37. 35 The rate of diffusion of a gas depends on the ____________ of the gas. Molar Mass Back

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