1. Unit 9 Review Gases

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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)

4. 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)

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

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

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

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)

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)

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

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

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

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

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

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

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

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)

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)

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

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

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

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

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)

24. 22 To two decimal places, what will v A /v B be equal to if N 2 is considered to be gas A and NO is considered to be gas B. (A diffusion problem) 1.03 (Diffusion)

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

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)

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

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)

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

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

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)

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

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

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

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

36. 34 T 1 = 76  C P 1 = 4 atmV 1 = 560 mL T 2 = 92  C P 2 = 2 atmV 2 = ? 1171 mL (PTV Chart)

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