Chemistry A Molecular Approach 3rd Edition By Nivaldo - Test Bank

Chemistry A Molecular Approach 3rd Edition By Nivaldo – Test Bank

 

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Sample Questions Are Posted Below

 

 

Chemistry: A Molecular Approach, 3e (Tro)

Chapter 5   Gases

 

Multiple Choice Questions

 

1) An instrument used to atmospheric pressure is called a

1. A) barometer
2. B) manometer
3. C) sphygmomanometer
4. D) spectrophotometer
5. E) spectrometer

Answer:  A

Diff: 1      Page Ref: 5.2

 

2) An instrument used to measure the pressure of a gas in a laboratory is called a

1. A) barometer
2. B) manometer
3. C) sphygmomanometer
4. D) spectrophotometer
5. E) spectrometer

Answer:  B

Diff: 1      Page Ref: 5.2

 

3) An instrument used to measure blood pressure is called a

1. A) barometer
2. B) manometer
3. C) sphygmomanometer
4. D) spectrophotometer
5. E) spectrometer

Answer:  C

Diff: 1      Page Ref: 5.2

 

4) The volume of a gas is proportional to the temperature of a gas is known as

1. A) Avogadro’s Law
2. B) Ideal Gas Law
3. C) Charles’s Law
4. D) Boyle’s Law
5. E) Dalton’s Law

Answer:  C

Diff: 1      Page Ref: 5.3

 

5) The volume of a gas is proportional to number of moles of a gas is known as

1. A) Avogadro’s Law
2. B) Ideal Gas Law
3. C) Charles’s Law
4. D) Boyle’s Law
5. E) Dalton’s Law

Answer:  A

Diff: 1      Page Ref: 5.3

 

6) The volume of a gas is inversely proportional to the pressure of a gas is known as

1. A) Avogadro’s Law
2. B) Ideal Gas Law
3. C) Charles’s Law
4. D) Boyle’s Law
5. E) Dalton’s Law

Answer:  D

Diff: 1      Page Ref: 5.3

 

7) A scuba diver experiences ________ as she descends into the ocean water.

1. A) decrease of 1 atm for each 20 m of depth
2. B) decrease of 1 atm for each 10 m of depth
3. C) increase of 1 atm for each 20 m of depth
4. D) increase of 1 atm for each 10 m of depth
5. E) no difference in pressure

Answer:  D

Diff: 1      Page Ref: 5.3

 

8) What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F2 has a volume of 25.0 mL at 1.2 atm?

1. A) 11 mL
2. B) 17 mL
3. C) 3.8 mL
4. D) 5.5 mL
5. E) 7.6 mL

Answer:  D

Diff: 2      Page Ref: 5.3

 

9) If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume will 0.66 moles occupy under the same conditions?

1. A) 12 L
2. B) 8.6 L
3. C) 17 L
4. D) 5.0 L
5. E) 15 L

Answer:  B

Diff: 2      Page Ref: 5.3

 

10) A syringe contains 0.65 moles of He gas that occupy 750.0 mL.  What volume (in L) of gas will the syringe hold if 0.35 moles of Ne is added?

1. A) 0.87 L
2. B) 4.9 L
3. C) 1.2 L
4. D) 2.1 L
5. E) 1.9 L

Answer:  C

Diff: 2      Page Ref: 5.3

 

 

11) To what temperature must a balloon, initially at 25°C and 2.00 L, be heated in order to have a volume of 6.00 L?

1. A) 993 K
2. B) 403 K
3. C) 75 K
4. D) 655 K
5. E) 894 K

Answer:  E

Diff: 3      Page Ref: 5.3

 

12) A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg.  What volume of gas will the balloon contain at 1.35 atm and 253 K?

22. A) 22.2 L
23. B) 87.5 L
24. C) 11.4 L
25. D) 45.0 L
26. E) 58.6 L

Answer:  D

Diff: 3      Page Ref: 5.3

 

13) A syringe initially holds a sample of gas with a volume of 285 mL at 355 K and 1.88 atm.  To what temperature must the gas in the syringe be heated/cooled in order to have a volume of 435 mL at 2.50 atm?

1. A) 139 K
2. B) 572 K
3. C) 175 K
4. D) 466 K
5. E) 721 K

Answer:  E

Diff: 3      Page Ref: 5.4

 

14) A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm.  What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?

10. A) 10.2 atm
11. B) 9.83 atm
12. C) 15.3 atm
13. D) 6.53 atm
14. E) 1.05 atm

Answer:  A

Diff: 3      Page Ref: 5.4

 

15) What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C?

4. A) 4.1 atm
5. B) 5.0 atm
6. C) 6.4 atm
7. D) 1.1 atm
8. E) 2.3 atm

Answer:  A

Diff: 3      Page Ref: 5.4

 

16) What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K?

18. A) 18.8 g
19. B) 53.1 g
20. C) 24.4 g
21. D) 86.7 g
22. E) 69.2 g

Answer:  D

Diff: 3      Page Ref: 5.4

 

17) What is the volume of 5.60 g of O2 at 7.78 atm and 415K?

1. A) 1.53 L
2. B) 565 L
3. C) 24.5 L
4. D) 25.0 L
5. E) 0.766 L

Answer:  E

Diff: 3      Page Ref: 5.4

 

18) Using the graph below, determine the gas that has the lowest density at STP.

 

 

1. A) A
2. B) B
3. C) C
4. D) D
5. E) All of the gases have the same density at STP.

Answer:  A

Diff: 1      Page Ref: 5.5

 

 

19) Using the graph below, determine the gas that has the highest density at STP.

 

 

1. A) A
2. B) B
3. C) C
4. D) D
5. E) All of the gases have the same density at STP.

Answer:  D

Diff: 1      Page Ref: 5.5

 

20) Which of the following will cause the volume of an ideal gas to triple in value?

1. A) Raising the temperature from 25°C to 75°C at constant pressure.
2. B) Lowering the absolute temperature by a factor of 3 at constant pressure.
3. C) Raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3.
4. D) Lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3.
5. E) Lowering the pressure by a factor of 3 while the temperature stays constant.

Answer:  E

Diff: 1      Page Ref: 5.5

 

21) Determine the density of CO2 gas at STP.

1. A) 1.96 g/L
2. B) 1.80 g/L
3. C) 2.24 g/L
4. D) 4.46 g/L
5. E) 5.10 g/L

Answer:  A

Diff: 2      Page Ref: 5.5

 

22) Determine the density of NH3 gas at 435 K and 1.00 atm.

2. A) 2.10 g/L
3. B) 0.477 g/L
4. C) 0.321 g/L
5. D) 2.24 g/L
6. E) 0.851 g/L

Answer:  B

Diff: 3      Page Ref: 5.5

 

23) A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm.  What is the identity of the halogen?

1. A) Br2
2. B) F2
3. C) Cl2
4. D) I2
5. E) Ge

Answer:  C

Diff: 3      Page Ref: 5.5

 

24) A 0.465 g sample of an unknown compound occupies 245 mL at 298 K and 1.22 atm.  What is the molar mass of the unknown compound?

26. A) 26.3 g/mol
27. B) 33.9 g/mol
28. C) 12.2 g/mol
29. D) 38.0 g/mol
30. E) 81.8 g/mol

Answer:  D

Diff: 3      Page Ref: 5.5

 

25) A compound is found to be 30.45% N and 69.55 % O by mass.  If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the molecular formula of the compound?

1. A) NO2
2. B) N2O
3. C) N4O2
4. D) N2O5
5. E) N2O4

Answer:  E

Diff: 4      Page Ref: 5.5

 

26) Define hypoxia.

1. A) oxygen starvation
2. B) increased oxygen concentration in body tissues
3. C) increased nitrogen concentration in body tissues and fluids
4. D) nitrogen starvation

Answer:  A

Diff: 1      Page Ref: 5.6

 

27) Define vapor pressure.

1. A) partial pressure of water in a liquid mixture
2. B) partial pressure of water in a gaseous mixture
3. C) condensation of water
4. D) water dissolved in a liquid
5. E) water molecules

Answer:  B

Diff: 1      Page Ref: 5.6

 

 

28) The total pressure of a gas mixture is the sum of the partial pressure of its components is known as

1. A) Avogadro’s Law
2. B) Ideal Gas Law
3. C) Charles’s Law
4. D) Boyle’s Law
5. E) Dalton’s Law

Answer:  E

Diff: 1      Page Ref: 5.6

 

29) A gas mixture consists of N2, O2, and Ne, where the mole fraction of N2 is 0.55 and the mole fraction of Ne is 0.25.  If the mixture is at STP in a 5.0 L container, how many molecules of O2 are present?

4. A) 4.5 × 1022 molecules O2
5. B) 2.7 × 1022molecules O2
6. C) 3.7 × 1023molecules O2
7. D) 1.1 × 1023molecules O2
8. E) 9.3 × 1024molecules O2

Answer:  B

Diff: 3      Page Ref: 5.6

 

30) A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm.  What is the partial pressure of Ne?

1. A) 1.1 atm
2. B) 0.80 atm
3. C) 0.54 atm
4. D) 0.40 atm
5. E) 1.3 atm

Answer:  A

Diff: 3      Page Ref: 5.6

 

31) The following reaction is used to generate hydrogen gas in the laboratory.  If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg, what mass of hydrogen is produced? A possibly useful table of water vapor pressures is provided below.

 

Mg(s) + 2 HCl(aq) →  MgCl2(aq) + H2(g)    T (°C)             P (mm Hg)

20                     17.55

25                     23.78

30                     31.86

 

1. A) 0.0196 g H2
2. B) 0.0717 g H2
3. C) 0.0190 g H2
4. D) 0.0144 g H2
5. E) 0.0449 g H2

Answer:  C

Diff: 3      Page Ref: 5.6

 

32) A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure.  A second syringe contains 473 mL of N2 at 298 K and 2.6 atm.  What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

1. A) 0.59 atm
2. B) 1.1 atm
3. C) 1.7 atm
4. D) 1.9 atm
5. E) 3.8 atm

Answer:  C

Diff: 5      Page Ref: 5.6

 

33) What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO2 at 398 K?

39. A) 39.6 atm
40. B) 7.02 atm
41. C) 32.6 atm
42. D) 46.6 atm
43. E) 58.7 atm

Answer:  D

Diff: 5      Page Ref: 5.6

 

34) Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction.  The molar mass for KClO3 is 122.55 g/mol.

 

2 KClO3(s) → 2 KCl(s) + 3 O2(g)

 

9. A) 9.14 L
10. B) 8.22 L
11. C) 12.3 L
12. D) 13.7 L
13. E) 14.6 L

Answer:  D

Diff: 4      Page Ref: 5.7

 

35) Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce 55.0 g of S.  Assume that there is excess SO2 present.

 

2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)

 

44. A) 44.0 L
45. B) 29.3 L
46. C) 22.7 L
47. D) 34.1 L
48. E) 66.0 L

Answer:  B

Diff: 4      Page Ref: 5.7

 

 

36) How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.60 atm) according to the following reaction?  Assume that there is excess Xe.

 

Xe(g) + 3 F2(g) → XeF6(g)

 

1. A) 1.21 × 1023molecules XeF6
2. B) 8.25 × 1023molecules XeF6
3. C) 2.75 × 1023molecules XeF6
4. D) 7.29 × 1023molecules XeF6
5. E) 1.37 × 1023molecules XeF6

Answer:  C

Diff: 4      Page Ref: 5.7

 

37) Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP).  The molar mass of KO2 = 71.10 g/mol and K2CO3 = 138.21 g/mol.

 

4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g)

 

27. A) 27.1 g, 80.4 % yield
28. B) 179 g, 12.2 % yield
29. C) 91.7 g, 23.8 % yield
30. D) 206 g, 10.6 % yield
31. E) 61.0 g, 35.7 % yield

Answer:  A

Diff: 4      Page Ref: 5.7

 

38) Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm).  The molar mass of FeS2 is 119.99 g/mol.

 

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)

 

36. A) 36.1 L
37. B) 45.3 L
38. C) 18.1 L
39. D) 27.6 L
40. E) 32.9 L

Answer:  E

Diff: 5      Page Ref: 5.7

 

 

39) Determine the mass of water formed when 12.5 L NH3 (at 298 K and 1.50 atm) is reacted with 18.9 L of O2 (at 323 K and 1.1 atm).

 

4 NH3(g) + 5 O2(g) →  4 NO(g) + 6 H2O(g)

 

17. A) 17.0 g H2O
18. B) 20.7 g H2O
19. C) 37.7 g H2O
20. D) 13.8 g H2O
21. E) 27.9 g H2O

Answer:  A

Diff: 5      Page Ref: 5.7

 

40) Determine the total volume of all gases (at STP) formed when 50.0 mL of TNT (C3H5(NO3)3, d = 1.60 g/mL, molar mass = 227.10 g/mol) reacts according to the following reaction.

 

4 C3H5(NO3)3(l) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g)

 

4. A) 4.93 L
5. B) 57.2 L
6. C) 29.6 L
7. D) 448 L
8. E) 175 L

Answer:  B

Diff: 5      Page Ref: 5.7

 

41) A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container.  Which of the following statements is TRUE?

1. A) Both gases have the same average kinetic energy.
2. B) Both gases contribute equally to the density of the mixture under these conditions.
3. C) Both gases have the same molecular speed.
4. D) The mixture has a volume of 22.4 L
5. E) All of the above are TRUE.

Answer:  A

Diff: 1      Page Ref: 5.8

 

42) Which statement is TRUE about kinetic molecular theory?

1. A) A single particle does not move in a straight line.
2. B) The size of the particle is large compared to the volume.
3. C) The collisions of particles with one another is completely elastic.
4. D) The average kinetic energy of a particle is not proportional to the temperature.

Answer:  C

Diff: 1      Page Ref: 5.8

 

 

43) Which of the gases in the graph below has the largest molar mass?

 

1. A) A
2. B) B
3. C) C
4. D) D
5. E) There is not enough information to determine.

Answer:  D

Diff: 2      Page Ref: 5.8

 

44) Calculate the root mean square velocity of nitrogen molecules at 25°C.

1. A) 729 m/s
2. B) 515 m/s
3. C) 149 m/s
4. D) 297 m/s

Answer:  B

Diff: 3      Page Ref: 5.8

 

45) The rate of effusion of two different gases is known as

1. A) Avogadro’s Law
2. B) Graham’s Law
3. C) Charles’s Law
4. D) Boyle’s Law
5. E) Dalton’s Law

Answer:  B

Diff: 1      Page Ref: 5.9

 

46) Give the definition for diffusion.

1. A) gas molecules mix equally
2. B) gas molecules spread out in a concentration gradient
3. C) gas molecules escape from a container into a vacuum through a small hole
4. D) average distance between collisions
5. E) gas molecules mix unequally

Answer:  B

Diff: 1      Page Ref: 5.9

 

 

47) The rate of effusion of oxygen to an unknown gas is 0.935.  What is the other gas?

1. A) Ne
2. B) Ar
3. C) F2
4. D) N2

Answer:  D

Diff: 3      Page Ref: 5.9

 

48) Which of the following statements is TRUE?

1. A) Particles of different masses have the same average speed at a given temperature.
2. B) The larger a molecule, the faster it will effuse.
3. C) At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law.
4. D) For a given gas, the lower the temperature, the faster it will effuse.
5. E) None of the above statements are true.

Answer:  C

Diff: 1      Page Ref: 5.10

 

49) Which of the following statements is TRUE?

1. A) At a given temperature, lighter gas particles travel more slowly than heavier gas particles.
2. B) The smaller a gas particle, the slower it will effuse
3. C) The higher the temperature, the lower the average kinetic energy of the sample.
4. D) At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law.
5. E) None of the above statements are true.

Answer:  D

Diff: 1      Page Ref: 5.10

 

50) Which of the following compounds will behave LEAST like an ideal gas at low temperatures?

1. A) He
2. B) SO2
3. C) H2
4. D) N2
5. E) F2

Answer:  B

Diff: 1      Page Ref: 5.10

 

51) This equation is used to calculate the properties of a gas under nonideal conditions.

1. A) Charles’s Law
2. B) Avogadro’s Law
3. C) Boyle’s Law
4. D) van der Waals equation
5. E) Dalton’s Law

Answer:  D

Diff: 1      Page Ref: 5.10

 

 

Algorithmic Questions

 

1) Convert 1.50 atm to mm Hg.

1. A) 760 mm Hg
2. B) 875 mm Hg
3. C) 1140 mm Hg
4. D) 1000 mm Hg
5. E) 1520 mm Hg

Answer:  C

Diff: 2      Page Ref: 5.2

 

2) Convert 1.50 atm to torr.

1. A) 760 torr
2. B) 875 torr
3. C) 1140 torr
4. D) 1000 torr
5. E) 1520 torr

Answer:  C

Diff: 2      Page Ref: 5.2

 

3) Convert 1.75 atm to psi.

52. A) 52.4 psi
53. B) 875 psi
54. C) 25.7 psi
55. D) 1000 psi
56. E) 1330 psi

Answer:  C

Diff: 2      Page Ref: 5.2

 

4) The atmospheric pressure is 700 mm Hg.  What is the pressure in inches of Hg?

16. A) 16.0 in Hg
17. B) 0.921 in Hg
18. C) 13.5 in Hg
19. D) 27.6 in Hg
20. E) 32.5 in Hg

Answer:  D

Diff: 3      Page Ref: 5.2

 

5) The atmospheric pressure is 715 mm Hg.  What is the pressure in torr?

1. A) 715 torr
2. B) 28.1 torr
3. C) 13.8 torr
4. D) 8 torr
5. E) 760 torr

Answer:  A

Diff: 2      Page Ref: 5.2

 

 

6) What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?

1. A) 656 mm Hg
2. B) 733 mm Hg
3. C) 751 mm Hg
4. D) 828 mm Hg

Answer:  A

Diff: 3      Page Ref: 5.2

 

7) If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg, the level of mercury in the tube will

1. A) be 118 mm higher in the arm open to the atmosphere.
2. B) be 118 mm higher in the arm connected to the gas cylinder.
3. C) be 870 mm higher in the arm open to the atmosphere.
4. D) be 870 mm higher in the arm connected to the gas cylinder.

Answer:  A

Diff: 3      Page Ref: 5.2

 

8) A container filled with gas is connected to an open-end manometer that is filled with mineral oil. The pressure in the gas container is 753 mm Hg and atmospheric pressure is 724 mm. How high will the level rise in the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively?

1. A) 1.75 mm
2. B) 23.8 mm
3. C) 29.0 mm
4. D) 480 mm

Answer:  D

Diff: 3      Page Ref: 5.2

 

9) What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 8.8 L at 4.4 atm?

2. A) 2.0 L
3. B) 0.50 L
4. C) 39 L
5. D) 13 L
6. E) 4.4 L

Answer:  C

Diff: 2      Page Ref: 5.3

 

10) A gas occupies 4.23 L at 2.25 atm.  What is the volume at 3.46 atm?

6. A) 6.50 L
7. B) 1.84 L
8. C) 2.75 L
9. D) 32.9 L
10. E) 0.364 L

Answer:  C

Diff: 2      Page Ref: 5.3

 

 

11) A sample of 0.200 moles of nitrogen occupies 0.400 L.  Under the same conditions, what number of moles occupies 1.200 L?

1. A) 0.600 moles
2. B) 0.0667 moles
3. C) 2.40 moles
4. D) 0.0960 moles

Answer:  A

Diff: 2      Page Ref: 5.3

 

12) To what volume will a sample of gas expand if it is heated from 50.0∘C and 2.33 L to 500.0°C?

5. A) 5.58 L
6. B) 23.3 L
7. C) 0.233 L
8. D) 0.97 L
9. E) 0.184 L

Answer:  A

Diff: 3      Page Ref: 5.3

 

13) A gas is at 35.0°C and 3.50 L.  What is the temperature at 7.00 L?

1. A) 343°C
2. B) 70.0°C
3. C) 616°C
4. D) 1.16°C
5. E) 17.5°C

Answer:  A

Diff: 3      Page Ref: 5.3

 

14) A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle’s law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

1. A) 846 torr
2. B) 0.118 torr
3. C) 5.26 × torr
4. D) 526 torr
5. E) 1.11 torr

Answer:  A

Diff: 2      Page Ref: 5.3

 

15) The volume of 350. mL of gas at 25°C is decreased to 135 mL at constant pressure. What is the final temperature of the gas?

1. A) -158°C
2. B) 9.6°C
3. C) 65°C
4. D) 500°C

Answer:  A

Diff: 3      Page Ref: 5.3

 

 

16) A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles’s law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

10. A) 10.9 L
11. B) 13.2 L
12. C) 2.07 L
13. D) 7.56 L
14. E) 48.4 L

Answer:  B

Diff: 2      Page Ref: 5.3

 

17) A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage. What is the pressure of the basketball outside where the temperature is -1.00°C?

1. A) 1.74 atm
2. B) 1.80 atm
3. C) 2.00 atm
4. D) 2.08 atm

Answer:  A

Diff: 3      Page Ref: 5.4

 

18) A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196°C, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the liquid nitrogen?

1. A) 0.25 L
2. B) 3.6 L
3. C) 6.7 L
4. D) 97 L

Answer:  A

Diff: 3      Page Ref: 5.4

 

19) What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25°C?

1. A) 0.35 atm
2. B) 4.1 atm
3. C) 4.7 atm
4. D) 8.6 atm
5. E) 3.6 atm

Answer:  B

Diff: 2      Page Ref: 5.4

 

20) How many moles of Ar are contained in a 5.00 L tank at 155°C and 2.80 atm?

1. A) 0.399 moles
2. B) 1.10 moles
3. C) 2.51 moles
4. D) 0.455 moles
5. E) 0.289 moles

Answer:  A

Diff: 2      Page Ref: 5.4

 

 

21) Calculate the temperature, in K, of 2.20 moles of gas occupying 3.30 L at 3.50 atm.

64. A) 64.0 K
65. B) -209 K
66. C) 337 K
67. D) 28.0 K

Answer:  A

Diff: 3      Page Ref: 5.4

 

22) What pressure will 2.6 x 1023 molecules of N2 exert in a 3.9 L container at 45°C?

5. A) 5.7 atm
6. B) 1.7 atm
7. C) 2.9 atm
8. D) 3.4 atm
9. E) 4.6 atm

Answer:  C

Diff: 3      Page Ref: 5.4

 

23) How many molecules of He  are contained in a 10.0 L tank at 7.53 atm and 485 K?

1. A) 1.89 × 1024molecules
2. B) 1.14 × 1024molecules
3. C) 8.32 × 1024molecules
4. D) 4.89 × 1024molecules
5. E) 3.63 × 1024molecules

Answer:  B

Diff: 3      Page Ref: 5.4

 

24) What is the volume of 9.783 x 1023 atoms of Kr at 9.25 atm and 512K?

7. A) 7.38 L
8. B) 3.69 L
9. C) 1.85 L
10. D) 15.4 L
11. E) 30.8 L

Answer:  A

Diff: 3      Page Ref: 5.4

 

25) How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C?

7. A) 7.01 × 1021 molecules
8. B) 7.38 × 1021 molecules
9. C) 2.12 × 1022 molecules
10. D) 2.23 × 1022 molecules

Answer:  B

Diff: 3      Page Ref: 5.4

 

 

26) A 55.0-L steel tank at 20.0°C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank?

3. A) 3.17 g
4. B) 8.20 g
5. C) 82.9 g
6. D) 1210 g

Answer:  C

Diff: 3      Page Ref: 5.4

 

27) What is the volume of 30.0 g of argon gas at 157°C and 2.50 kPa pressure?

3. A) 3.87 L
4. B) 10.6 L
5. C) 393 L
6. D) 1070 L

Answer:  D

Diff: 3      Page Ref: 5.4

 

28) What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?

1. A) -23°C
2. B) 228°C
3. C) 250°C
4. D) 500°C

Answer:  B

Diff: 3      Page Ref: 5.4

 

29) A gas bottle contains 0.250 mol of gas at 730 mm Hg pressure. If the final pressure is 1.15 atm, how many moles of gas were added to the bottle?

1. A) 0.0262 mol
2. B) 0.0493 mol
3. C) 0.276 mol
4. D) 0.299 mol

Answer:  B

Diff: 3      Page Ref: 5.4

 

30) A 2.75-L container filled with CO2 gas at 25°C and 225 kPa pressure springs a leak. When the container is re-sealed, the pressure is 185 kPA and the temperature is 10°C. How many moles of gas were lost?

1. A) 0.0335 mol
2. B) 0.728 mol
3. C) 0.882 mol
4. D) 3.39 mol

Answer:  A

Diff: 3      Page Ref: 5.4

 

 

31) How many grams of F2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C?

19. A) 19.5 g
20. B) 41.1 g
21. C) 500 g
22. D) 2.96 × 104g

Answer:  B

Diff: 3      Page Ref: 5.4

 

32) A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?

1. A) 0.319 atm
2. B) 1.05 atm
3. C) 1.44 atm
4. D) 1.96 atm

Answer:  B

Diff: 4      Page Ref: 5.4

 

33) Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains C2H4, flask B contains O3, and flask C contains F2. Which flask contains the largest number of molecules?

1. A) flask A
2. B) flask B
3. C) flask C
4. D) All contain same number of molecules.

Answer:  D

Diff: 1      Page Ref: 5.5

 

34) The density of nitric oxide (NO) gas at 1.21 atm and 54.1°C is ________ g/L.

1. A) 0.0451
2. B) 0.740
3. C) 1.35
4. D) 0.273
5. E) 8.2

Answer:  C

Diff: 3      Page Ref: 5.5

 

35) The density of krypton gas at 1.21 atm and 50.0°C is ________ g/L.

1. A) 0.0456
2. B) 0.262
3. C) 0.295
4. D) 3.82
5. E) 7.65

Answer:  D

Diff: 3      Page Ref: 5.5

 

 

36) Give the temperature and pressure at STP.

1. A) 0°C and 1.00 atm
2. B) 0K and 1.00 atm
3. C) 25°C and 1.00 in Hg
4. D) 32K and 1 torr Hg
5. E) 0°C and 1 mm Hg

Answer:  A

Diff: 1      Page Ref: 5.5

 

37) Which of the following gas samples would be most likely to behave ideally under the stated conditions?

1. A) Ar at STP
2. B) CO at 200 atm and 25°C
3. C) SO2at 2 atm and 0 K
4. D) N2at 1 atm and -70°C
5. E) H2at 400 atm and 25°C

Answer:  A

Diff: 1      Page Ref: 5.5

 

38) Which of the following samples will have the greatest volume at STP?

1. A) 22 g Ne
2. B) 22 g He
3. C) 22 g O2
4. D) 22 g Cl2
5. E) All of these samples would have the same volume at STP.

Answer:  B

Diff: 1      Page Ref: 5.5

 

39) Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?

1. A) 15 g H2
2. B) 15 g Ar
3. C) 15 g Kr
4. D) 15 g CO2
5. E) All of these samples will have the same pressure.

Answer:  C

Diff: 1      Page Ref: 5.5

 

40) Which of the following samples has the greatest density at STP?

1. A) NO2
2. B) Xe
3. C) SO2
4. D) SF6
5. E) All of these samples have the same density at STP.

Answer:  D

Diff: 1      Page Ref: 5.5

 

 

41) Place the following gases in order of increasing density at STP.

 

F2        NH3    N2O4  Ar

 

1. A) N2O4 < Ar  <  F2  <  NH3
2. B) Ar < N2O4  <  F2  <  NH3
3. C) F2 < Ar  <  N2O4  <  NH3
4. D) NH3 < F2  <  Ar <  N2O4
5. E) Ar < F2  <  NH3  <  N2O4

Answer:  D

Diff: 1      Page Ref: 5.5

 

42) The density of a gas is 3.16 g/L at STP.  What is the gas?

1. A) H2
2. B) Br2
3. C) Kr
4. D) Cl2
5. E) Ar

Answer:  D

Diff: 2      Page Ref: 5.5

 

43) What volume will 4.91 x 1022 atoms of Ar occupy at STP?

1. A) 1.10 L
2. B) 2.00 L
3. C) 2.24 L
4. D) 3.11 L
5. E) 1.83 L

Answer:  E

Diff: 3      Page Ref: 5.5

 

44) What volume will 0.780 moles of Xe occupy at STP?

22. A) 22.4 L
23. B) 70.0 L
24. C) 43.7 atm
25. D) 17.5 L
26. E) 15.6 L

Answer:  D

Diff: 3      Page Ref: 5.5

 

45) A steel bottle contains argon gas at STP. What is the final pressure if the temperature is changed to 145°C?

1. A) 0.653 atm
2. B) 0.713 atm
3. C) 1.40 atm
4. D) 1.53 atm

Answer:  D

Diff: 3      Page Ref: 5.5

 

 

46) A gas occupies 22.4 L at STP and 19.0 L at 100°C and 1.50 atm pressure. How many moles of gas did the system gain or lose?

1. A) 0.08 moles gained
2. B) 0.01 moles gained
3. C) 0.01 moles lost
4. D) 07 moles lost

Answer:  D

Diff: 3      Page Ref: 5.5

 

47) What is the density of hydrogen gas at STP?

11. A) 11.1 g/L
12. B) 0.0450 g/L
13. C) 0.0823 g/L
14. D) 0.0899 g/L

Answer:  D

Diff: 3      Page Ref: 5.5

 

48) Which of the following would have a density of 1.37 g/L at 7.0°C and 0.987 atm?

1. A) N2
2. B) O2
3. C) Kr
4. D) Rn

Answer:  B

Diff: 3      Page Ref: 5.5

 

49) The density of chlorine gas at 1.21 atm and 34.9°C is ________ g/L.

1. A) 0.0479
2. B) 0.295
3. C) 0.423
4. D) 1.70
5. E) 3.39

Answer:  E

Diff: 3      Page Ref: 5.5

 

50) A 0.286-g sample of gas occupies 125 mL at 60. cm of Hg and 25°C. What is the molar mass of the gas?

5. A) 5.9 g/mol
6. B) 44 g/mol
7. C) 59 g/mol
8. D) 71 g/mol

Answer:  D

Diff: 3      Page Ref: 5.5

 

 

51) Given three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at -15°C, cylinder B is at -5°F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen?

1. A) cylinder A
2. B) cylinder B
3. C) cylinder C
4. D) All cylinders contain the same mass of O2.

Answer:  B

Diff: 3      Page Ref: 5.5

 

52) A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is ________.

1. A) argon
2. B) helium
3. C) krypton
4. D) neon
5. E) xenon

Answer:  E

Diff: 4      Page Ref: 5.5

 

53) Give the gas that is the lowest percent by volume in dry gas.

1. A) CO2
2. B) He
3. C) H2
4. D) N2

Answer:  A

Diff: 1      Page Ref: 5.6

 

54) In a container containing CO, H2, and O2, what is the mole fraction of CO if the H2 mole fraction is 0.22 and the O2 mole fraction is 0.58?

1. A) 0.20
2. B) 0.30
3. C) 0.10
4. D) 0.50

Answer:  A

Diff: 1      Page Ref: 5.6

 

55) A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total pressure of 2.95 atm.  What is the pressure of H2?

1. A) 1.17 atm
2. B) 0.853 atm
3. C) 1.03 atm
4. D) 0.969 atm
5. E) 0.649 atm

Answer:  B

Diff: 2      Page Ref: 5.6

 

 

56) A mixture of 0.220 moles CO, 0.350 moles N2 and 0.640 moles Ne has a total pressure of 2.95 atm.  What is the pressure of CO?

1. A) 1.86 atm
2. B) 0.649 atm
3. C) 0.536 atm
4. D) 1.54 atm
5. E) 0.955 atm

Answer:  C

Diff: 2      Page Ref: 5.6

 

57) A mixture of N2, O2 and He have mole fractions of 0.25, 0.65, and 0.10, respectively.  What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?

2. A) 2.5 atm
3. B) 0.39 atm
4. C) 0.67 atm
5. D) 0.98 atm
6. E) 1.33 atm

Answer:  D

Diff: 2      Page Ref: 5.6

 

58) A mixture of Ar, Ne and He has a pressure of 7.85 atm.  If the Ne has a mole fraction of 0.47 and He has a mole fraction of 0.23, what is the pressure of Ar?

4. A) 4.2 atm
5. B) 3.7 atm
6. C) 1.8 atm
7. D) 5.5 atm
8. E) 2.4 atm

Answer:  E

Diff: 2      Page Ref: 5.6

 

59) A gas mixture contains CO, Ar and H2.  What is the total pressure of the mixture, if the mole fraction of H2 is 0.350 and the pressure of H2 is 0.480 atm?

1. A) 1.37 atm
2. B) 0.168 atm
3. C) 5.95 atm
4. D) 0.729 atm
5. E) 2.1 atm

Answer:  A

Diff: 3      Page Ref: 5.6

 

60) The mole fraction of argon in dry air near sea level is 1.818 × 10-5 where the molar mass of argon is 39.948. The concentration of argon in the atmosphere is ________ ppm.

1. A) 1.07 × 108
2. B) 0.934
3. C) 9.34 × 106
4. D) 18.18
5. E) 9.34 × 109

Answer:  D

Diff: 2      Page Ref: 5.6

 

61) A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He and 0.026 mol H2 at 749 mm Hg. What is the partial pressure of O2?

1. A) 20 mm Hg
2. B) 23 mm Hg
3. C) 140 mm Hg
4. D) 570 mm Hg

Answer:  C

Diff: 3      Page Ref: 5.6

 

62) What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C?

1. A) 0.510 atm
2. B) 0.681 atm
3. C) 1.16 atm
4. D) 1.66 atm

Answer:  D

Diff: 3      Page Ref: 5.6

 

63) The concentration of water vapor in a sample of air that has a partial pressure of water of 0.91 torr and a total pressure of air of 735 torr is ________ ppm.

1. A) 1.2 × 103
2. B) 1.2
3. C) 0.12
4. D) 8.1 × 10-4
5. E) 0.81

Answer:  A

Diff: 3      Page Ref: 5.6

 

64) A sample of air from a home is found to contain 6.2 ppm of carbon monoxide.  This means that if the total pressure is 695 torr, then the partial pressure of CO is ________ torr.

4. A) 4.3 × 103
5. B) 4.3 × 10-3
6. C) 4.3
7. D) 8.9 × 103
8. E) 1.1 × 108

Answer:  B

Diff: 3      Page Ref: 5.6

 

65) The concentration of ozone in a sample of air that has a partial pressure of  of 0.33 torr and a total pressure of air of 735 torr is ________ ppm.

4. A) 4.5 × 102
5. B) 0.45
6. C) 0.045
7. D) 2.2 × 10-3
8. E) 2.2

Answer:  A

Diff: 3      Page Ref: 5.6

 

66) The mole fraction of carbon dioxide in dry air near sea level is 0.000375, where the molar mass of carbon dioxide is 44.010. The partial pressure of carbon dioxide when the total atmospheric pressure (dry air) is 97.5 kPa is ________ kPa.

2. A) 2.63 × 105
3. B) 5.97 × 103
4. C) 0.0370
5. D) 1.63
6. E) 8.40 × 10-4

Answer:  C

Diff: 3      Page Ref: 5.6

 

67) In the laboratory, hydrogen gas is usually made by the following reaction:

Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq)

How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 3.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C.

1. A) 0.0975 L
2. B) 1.30 L
3. C) 1.33 L
4. D) 1.36 L

Answer:  D

Diff: 4      Page Ref: 5.6

 

68) A 0.600 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation:

2 Ag2O(s) → 4 Ag(s) + O2(g)

If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mm Hg at 27°C.

10. A) 10.4%
11. B) 20.9%
12. C) 41.8%
13. D) 44.8%

Answer:  C

Diff: 4      Page Ref: 5.6

 

 

69) Zinc reacts with aqueous sulfuric acid to form hydrogen gas:

 

Zn(s) + H2SO4 (aq)  →  ZnSO4 (aq) + H2 (g)

 

In an experiment, 225 mL of wet H2 is collected over water at 27°C and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27°C is 26.74 torr.

4. A) 4.79 × 106
5. B) 0.567
6. C) 567
7. D) 431
8. E) 4.31 × 105

Answer:  B

Diff: 4      Page Ref: 5.6

 

70) Zinc reacts with aqueous sulfuric acid to form hydrogen gas:

 

Zn(s) + H2SO4 (aq)  →  ZnSO4 (aq) + H2 (g)

 

In an experiment, 201 mL of wet H2 is collected over water at 27°C and a barometric pressure of 733 torr. The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is ________ atm.

1. A) 0.929
2. B) 706
3. C) 0.964
4. D) 760
5. E) 1.00

Answer:  A

Diff: 4      Page Ref: 5.6

 

71) The mole fraction of oxygen in dry air near sea level is 0.20948. The concentration of oxygen is ________ molecules per liter, assuming an atmospheric pressure of 739 torr and a temperature of 29.5°C.

6. A) 6.23
7. B) 0.00819
8. C) 4.93 × 1021
9. D) 3.75 × 1024
10. E) 5.07 × 1022

Answer:  C

Diff: 5      Page Ref: 5.6

 

 

72) The concentration of carbon monoxide in a sample of air is 9.2 ppm. There are ________ molecules of CO in 1.00 L of this air at 755 torr and 23°C.

3. A) 3.8 × 10-7
4. B) 2.2 × 1021
5. C) 2.9 × 1018
6. D) 1.7 × 1020
7. E) 2.3 × 1017

Answer:  E

Diff: 5      Page Ref: 5.6

 

73) The action of some commercial drain cleaners is based on the following reaction:

2 NaOH(s) + 2 Al(s) + 6 H2O(l) → 2 NaAl(OH)4(s) + 3 H2(g)

What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH?

3. A) 3.50 L
4. B) 5.25 L
5. C) 7.87 L
6. D) 8.59 L

Answer:  C

Diff: 5      Page Ref: 5.7

 

74) How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l)

13. A) 13.9 L
14. B) 27.8 L
15. C) 55.5 L
16. D) 60.5 L

Answer:  C

Diff: 5      Page Ref: 5.7

 

75) When 14.0 g of zinc metal reacts with excess HCl, how many liters of H2 gas are produced at STP?

1. A) 0.208 L
2. B) 0.416 L
3. C) 4.80 L
4. D) 9.60 L

Answer:  C

Diff: 5      Page Ref: 5.7

 

76) How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below?

XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g)

9. A) 9.58 g
10. B) 11.7 g
11. C) 35.2 g
12. D) 106 g

Answer:  B

Diff: 5      Page Ref: 5.7

 

 

77) A 1.000 kg sample of nitroglycerine, C3H5N3O9, explodes and releases gases with a temperature of 1985°C at 1.100 atm. What is the volume of gas produced?

4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)

742. A) 742.2 L
743. B) 3525 L
744. C) 4730 L
745. D) 5378 L

Answer:  D

Diff: 5      Page Ref: 5.7

 

78) Calcium hydride (CaH2) reacts with water to form hydrogen gas:

 

CaH2(s) + 2H2O(l)  →  Ca(OH)2(aq) + 2H2(g)

 

How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.888 atm and a temperature of 32°C?

50. A) 50.7
51. B) 0.851
52. C) 143
53. D) 35.8
54. E) 71.7

Answer:  D

Diff: 5      Page Ref: 5.7

 

79) How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below?

Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)

1. A) 0.171 g
2. B) 5.83 g
3. C) 11.7 g
4. D) 131 g

Answer:  B

Diff: 5      Page Ref: 5.7

 

80) How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below?

CaH2(s) + 2 H2O(l) → Ca(OH)2(aq) + 2 H2(g)

3. A) 3.82 g
4. B) 7.64 g
5. C) 15.3 g
6. D) 45.6 g

Answer:  A

Diff: 5      Page Ref: 5.7

 

 

81) How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°C and 755 mm Hg pressure according to the chemical equation shown below?

BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g)

1. A) 0.219 L
2. B) 0.799 L
3. C) 1.60 L
4. D) 3.21 L

Answer:  D

Diff: 5      Page Ref: 5.7

 

82) How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below?

BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g)

2. A) 2.01 g
3. B) 4.02 g
4. C) 4.07 g
5. D) 8.04 g

Answer:  B

Diff: 5      Page Ref: 5.7

 

83) How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below?

2 H2(g) + O2(g) → 2 H2O(l)

67. A) 67.9 L
68. B) 136 L
69. C) 203 L
70. D) 407 L

Answer:  B

Diff: 5      Page Ref: 5.7

 

84) What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below?

2 H2O(l) → 2 H2(g) + O2(g)

74. A) 74.7 L
75. B) 149 L
76. C) 224 L
77. D) 447 L

Answer:  C

Diff: 5      Page Ref: 5.7

 

 

85) How many mL of O2 gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO3(s) according to the chemical equation shown below?

2 KClO3(s) → 2 KCl(s) + 3 O2(g)

30. A) 30.1 mL
31. B) 40.2 mL
32. C) 90.4 mL
33. D) 181 mL

Answer:  C

Diff: 5      Page Ref: 5.7

 

86) How many grams of KCl(s) are produced from the thermal decomposition of KClO3(s) which produces 50.0 mL of O2(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below?

2 KClO3(s) → 2 KCl(s) + 3 O2(g)?

1. A) 0.102 g
2. B) 0.152 g
3. C) 0.167 g
4. D) 0.304 g

Answer:  A

Diff: 5      Page Ref: 5.7

 

87) How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H2O2 in the reaction according to the chemical equation shown below?

2 H2O2(l) → 2 H2O(l) + O2(g)

8. A) 8.41 L
9. B) 11.2 L
10. C) 16.8 L
11. D) 33.6 L

Answer:  A

Diff: 5      Page Ref: 5.7

 

88) What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.0425 grams of H2O2 at 700°C and 755 mm Hg according to the chemical equation shown below?

H2O2(l) → H2(g) + O2(g)?

50. A) 50.2 mL
51. B) 100 mL
52. C) 151 mL
53. D) 201 mL

Answer:  D

Diff: 5      Page Ref: 5.7

 

 

89) How many liters of O2 gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below?

2 KH(s) + O2(g) → H2O(l) + K2O(s)

9. A) 9.19 L
10. B) 18.4 L
11. C) 36.8 L
12. D) 73.5 L

Answer:  B

Diff: 5      Page Ref: 5.7

 

90) How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0.100 M aqueous solution of KI according to the chemical equation shown below?

O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(s) + 2 OH-(aq)

55. A) 55.0 mL
56. B) 110. mL
57. C) 165 mL
58. D) 220. mL

Answer:  A

Diff: 5      Page Ref: 5.7

 

91) Identify the gas particle that travels the fastest.

1. A) H2
2. B) N2
3. C) Ne
4. D) Cl2
5. E) CO

Answer:  A

Diff: 1      Page Ref: 5.8

 

92) Identify the gas particle that travels the slowest.

1. A) H2
2. B) N2
3. C) Ne
4. D) F2
5. E) CO

Answer:  E

Diff: 1      Page Ref: 5.8

 

93) What is the average speed (actually the root-mean-square speed) of a neon atom at 27°C?

5. A) 5.78 m/s
6. B) 19.3 m/s
7. C) 183 m/s
8. D) 609 m/s

Answer:  D

Diff: 3      Page Ref: 5.8

 

 

94) Which of the following gases has the highest average speed at 400K?

1. A) N2
2. B) O2
3. C) F2
4. D) Cl2

Answer:  A

Diff: 3      Page Ref: 5.8

 

95) Which of the following gases has the lowest average speed at 25°C?

1. A) C3H8
2. B) Kr
3. C) CH3NH2
4. D) SO2

Answer:  B

Diff: 3      Page Ref: 5.8

 

96) What is the temperature of NO2 gas if the average speed (actually the root-mean-square speed) of the molecules is 750 m/s?

1. A) 1.38 K
2. B) 1.04 × 103K
3. C) 1.38 × 103K
4. D) 1.04 × 106K

Answer:  B

Diff: 3      Page Ref: 5.8

 

97) If NO  and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of effusion for NH3 will be ________ times that of NO .

1. A) 0.57
2. B) 0.75
3. C) 1.3
4. D) 1.8

Answer:  C

Diff: 3      Page Ref: 5.9

 

98) Rank the following in order of decreasing rate of effusion.

 

F2        SF6      He       Ar

 

1. A) SF6 > Ar  >  F2  >  He
2. B) Ar > He  >  SF6  >  F2
3. C) F2 > Ar  >  He  >  SF6
4. D) He > F2  >  Ar  >  SF6
5. E) He > F2  >  SF6 >  Ar

Answer:  D

Diff: 1      Page Ref: 5.9

 

 

99) Calculate the ratio of effusion rates of Cl2 to O2.

47. A) 47.7
48. B) 0.451
49. C) 2.22
50. D) 1.49
51. E) 0.671

Answer:  E

Diff: 2      Page Ref: 5.9

 

100) A sample of N2 effuses in 220 s.  How long will the same size sample of Cl2 take to effuse?

1. A) 350 s
2. B) 138 s
3. C) 558 s
4. D) 86.8 s
5. E) 388 s

Answer:  A

Diff: 3      Page Ref: 5.9

 

101) Which of the following samples will have the greatest average speed at 355 K?

1. A) Kr
2. B) C2H4
3. C) Cl2
4. D) CH4
5. E) All of these samples will have the same average speed at the same temperature.

Answer:  D

Diff: 1      Page Ref: 5.9

 

 

Matching Questions

 

Match the following.

 

1. A) V1/n1= V2/n2
2. B) measures atmospheric pressure
3. C) measures pressure of a gas in the laboratory
4. D) PT= PA+ PB + PC …
5. E) V1/T1= V2/T2
6. F) measures blood pressure
7. G) PV = nRT
8. H) P1V1= P2V2

 

1) barometer

Diff: 1      Page Ref: 5.2

 

2) manometer

Diff: 1      Page Ref: 5.2

 

3) sphygmomanometer

Diff: 1      Page Ref: 5.2

 

4) Boyle’s Law

Diff: 1      Page Ref: 5.3

 

5) Charles’s Law

Diff: 1     Page Ref: 5.3

 

6) Avogadro’s Law

Diff: 1      Page Ref: 5.3

 

7) Ideal Gas Law

Diff: 1      Page Ref: 5.4

 

8) Dalton’s Law

Diff: 1      Page Ref: 5.6

 

Answers: 1) B  2) C  3) F  4) H  5) E  6) A  7) G  8) D

 

 

 

Short Answer Questions

 

1) Define pressure.

Answer:  Pressure is the force exerted per unit area by gas molecules as they strike the surfaces around them.

Diff: 1      Page Ref: 5.1

 

2) Consider a container of gas under a particular P, V, T set of conditions.  Describe how the pressure would change if the volume were doubled while the absolute temperature was increasing by a factor of two.

Answer:  The pressure would stay constant.  The doubling of the volume would, by itself, decrease the pressure by a factor of 2.  However, the temperature is also decreasing by a factor of 2.  These two changing variables will cancel one another.

Diff: 2      Page Ref: 5.3

 

3) Why does HOT air rise?

Answer:  As air is heated, it expands and becomes less dense (the same mass of air fills a larger volume).  This lower density warm air will “float” to the top of cooler, more dense air.

Diff: 1      Page Ref: 5.5

 

4) Give the major gas in dry air.

Answer:  nitrogen

Diff: 1      Page Ref: 5.6

 

5) Why doesn’t Dalton’s Law of Partial Pressures depend on the identity of the gases present?

Answer:  It is assumed that all gas particles are behaving ideally and not interacting with one another.  If that is true, the only difference between particles is associated with their mass.  Since all of the gases are at the same temperature and have the same average kinetic energy, their masses don’t have to be taken into account.  All that matters is all of the different gas particles exert the same force on the walls of the container, no matter what their mass.

Diff: 1      Page Ref: 5.6

 

6) Given the equation C2H6(g) + O2(g) →  CO2(g) + H2O(g)  (not balanced), determine the number of liters of CO2 formed at STP when 240.0 grams of C2H6 is burned in excess oxygen gas.

Answer:  358

Diff: 5      Page Ref: 5.7

 

7) Given the equation C2H6(g) + O2(g) → CO2(g) + H2O(g)  (not balanced), determine the number of liters of O2 consumed at STP when 270.0 grams of C2H6 is burned.

Answer:  706

Diff: 5      Page Ref: 5.7

 

8) Explain what the term “mean free path” describes.  How does it change with decreasing pressure?

Answer:  Mean free path describes the distance that a gas particle can travel before hitting another particle.  As pressure decreases, the distance between particles increases, therefore increasing the mean free path of the particles.

Diff: 1      Page Ref: 5.9

 

 

9) Why does the rate of effusion increase with a decrease in the molar mass?

Answer:  The rate of effusion depends on the speed of the gas particles.  As the molar mass decreases at a given temperature, the average speed of the particles increases, increasing the rate of effusion.

Diff: 1      Page Ref: 5.9

 

10) Define effusion.

Answer:  Effusion is the process by which a gas escapes from a container into a vacuum through a small hole.

Diff: 1      Page Ref: 5.9