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1. Which of the following is a correct interpretation of the ideal gas law?

2. What is the correct relationship between vrms, , and vp?

3. An isolated container of gas doubles in pressure and triples in volume. By what factor does T change?

4. If the volume of a gas is doubled at constant temperature, the factor by which the pressure increases is:

5. A barometer filled with an unknown liquid has a height of 1 m at 1 atm. During stormy weather, the height of the column is observed to rise to 1.3 m. What is the atmospheric pressure?

6. Which of the following are possible units of R?

7.
You take a reading of 760 mm of Hg at 0 degrees Celsius. However, you realize that the volume at the top of the barometer is not a complete vacuum. There is some Hg vapor above the Hg column! If the pressure of Hg is 10 mm Hg, what is the actual atmospheric pressure?

8. What are the conditions of STP?

9. A container contains 32 grams of O2 gas and 2 grams of H2 gas. If the total pressure of the vessel is 16 atm, what is the partial pressure of the H2 gas?

10. As the average radius of a population of gas molecules increases, how does the factor b of van der Waals equation change?

11. All of the following are properties of an ideal gas except:

12. The ideal gas law is most valid under these conditions:

13. The reaction

N2 +2O2→2NO2    

1 mol of N2 and 2 mol O2 react completely in an isolated, rigid container with initial pressure 1 atm. The temperature does not change. What is the pressure inside the container after the reaction has gone to completion?

14.
There are 4.0 mol of gas a in container A at 1.0 atm and 273 K. There are 2.0 mol of gas b in container B at 2.0 atm and 273 K. What is the total volume of containers A and B?

15.

   

Is the equation for:

16. For the van der Waals equation:

(P + )(V - nb) = nRT    

The value "b" corrects for:

17. For the equation PV = nRT, the value of T must be expressed in:

18. Which of the following is not a SI unit

19. A sample of gas has a volume of 22.4 L at a temperature of 273 K. How many moles are in the sample?

20. The volume of a sample of gas expands five times at constant pressure. By what factor has the absolute temperature changed?

21. The following reaction produces H2O gas:

2H2 + O2→2H2O    

64.0 g of O_2 are used and an excess of H2, and the reaction goes to completion. How many liters of H2O gas will be generated if the pressure is 2.0 atm and the temperature is 273 K?

22. A sample of gas occupies 100 L at STP. If the absolute temperature is halved while all other conditions are constant, what will be the final volume?

23. Calculate the vrms of a sample of O2 at 300 K.

24. A closed jar contains 2 moles of O2 and 3 moles of N2. What is the ratio of the partial pressure of the O2 over the total pressure in the jar?

25. The rate of effusion of gas A is four times that of gas B. What is ?

26.
The Hg containing dish of the barometer is replaced with one four times its diameter. By what factor does H change?

27. The density of a certain gas at STP is 1.43 g/L. What is the identity of the gas?

28. One end of a mercury manometer is open to the atmosphere (Patm = 760mmHg). The other end is connected to a 1 mol sample of CH4 that is at 273 K and occupies 22.4 L. What is the height of the mercury column?

29. The Maxwell-Boltzmann distribution graph plots:

30. James the giant has big shoes to fill. His shoes have a total area of 20m2 in contact with the ground. Unfortunately, James' feet are not so big. Barefoot, his weight is spread over 1m2. What is the ratio of the pressure he exerts on the ground barefoot over the pressure he exerts with his shoes on?

31. The "air" in airbags is generated via the decomposition of solid NaN3:

2NaN3→2Na + 3N2    

2/3 mole of solid NaN3 are completely decomposed at a temperature of 300 K. In order for the final pressure in the airbag to be 1.2 atm, what must the final volume of the bag be in L? Assume that the Na takes up no appreciable volume. R = 0.0821.

32. A sample of an ideal gas is compressed at constant temperature. What happens to the average kinetic energy of the molecules?

33. A piston compresses a gas at constant temperature. Initially the gas occupied 1 L and was at a pressure of 1 atm. After compression, the gas occupies 0.1 atm. What is the pressure of the compressed gas?

34. A collaborator from a foreign country reports that the value of R as 8. He has probably used units of "woozle" for which of the following variables:

35. Avogadro's number is:

36. What is

   

if both samples of gas are at the same temperature?

37. The following Maxwell-Boltzmann distribution plot was measured for two gases A and B at the same temperature:
Which gas has the greater molecular mass?

38. A rigid container holds a mixture of gases. Within this mixture, the partial pressure of O2 is 400 torr. If an additional quantity of N2 gas is injected into the container such that the total pressure of the container rises by 760 torr, what is the change in the partial pressure of O2? Assume that the temperature of the container's contents stays constant.

39. If the pressure of a gas doubles and the temperature quadruples, by what factor does the volume change?

40. Which of the following are possible units for pressure?

41. The following Maxwell-Boltzmann distribution plot was measured for a gas at two temperatures A and B:
What is the relationship between A and B?

42. For the following calculation of vrms, the molar mass (MM) should be expressed in what units?


vrms=  
 = sqrt  

43. By what significant numerical value are Boltzmann's constant (k) and the gas constant (R) related?

44. The pressure of a gas is tripled while the volume is halved. By what factor does the temperature increase?

45. The gas constant R:

46. One end of a manometer is sealed off to a vacuum. The other end of the manometer is connected to a pressurized gas. The height of the liquid column is indicative of:

47. A sample of O2 and a sample of N2 both have a temperature of 330 K. What is the ratio of the average kinetic energy of the O2 over that of the N2?

48. The density of a gas at STP is 0.089 g/L. What is the molar mass of the gas?

49. The following Maxwell-Boltzmann distribution plot was measured for two gases A and B at temperatures TA and TB:
Which gas has the greater molar mass?

50. Gaseous methane (CH4) burns completely in gaseous oxygen to produce carbon dioxide gas and water vapor.

CH4 +2O2→CO2 + 2HOH    

2 mole of CH4 and 4 moles of O2 completely react in a closed vessel. If temperature and volume are constant, by what factor will pressure increase?

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